Name: _____________________
Unit 2:1
Properties of Matter
Period: _____________________
Hardness
How difficult it is to
scratch something.
A diamond is very hard
because you can’t scratch it.
Glass is brittle because it
will easily shatter if dropped.
Soap is easy to
scratch, so it is not hard.
Elasticity
Wood is not very brittle
because it will not shatter if dropped.
How much something can bend
and return to its original shape.
A pencil is not elastic because
it will break if you bend it.
Gold is very malleable because you
can pound it into very thin sheets.
Ice is not malleable because
it will shatter instead of spread out.
How slowly a liquid pours.
Tensile Strength
Tissue paper is easily pulled apart,
so it has very little tensile strength..
Water pours quickly,
so it is not viscous.
Density is how compact an object is. Density is a measure of how tightly packed the
atoms of a substance are. More tightly packed atoms make a denser substance.
If two objects have the same
size (volume) the one with
more mass is denser.
30 g
A ping-pong ball and a golf
ball are approximately the
same size, but the golf ball
is heavier, so it is denser.
in g/mL or
g/cm3
D= m
v
Volume in
cm3 or mL
Density = Mass ÷ Volume
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If two objects have the same
mass the smaller one
(less volume) is denser.
10 g
30 g
This one
is denser.
Mass in grams (g)
Density:
How hard it is to break
something by pulling it.
Spider webs can be pulled very hard before
they break. Spider webs have more tensile
strength than steel cables.
Syrup pours very slowly,
so it is very viscous.
Density
How easy it is to pound
something into thin sheets.
Malleability
Rubber is very elastic because
it can stretch without breaking.
Viscosity
How easy it is to shatter
when dropped or struck.
Brittleness
30 g
This one
is denser.
D= m
v
is a formula. Put the number in the correct part of the formula to find density.
Ex. An 20 gram object has a volume of 5 cm3.
Find its density.
Solution:
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D=
m 20 g
g
=
=4 3
3
V 5cm
cm
Copyright © 2006, C. Stephen Murray
Name: _____________________
Unit 2:1
Period: _____________________
1. Density
a. A measurement of how easily a solid can
be pounded into thin sheets
1.Tensile
Strength
2. Hardness
b. A measurement of the “compactness” of
a substance; ratio of mass to volume.
2. viscosity
3. Brittleness
c. Measure of a solid’s ability to return to
its original shape after stretching.
3. cm3
C. Measure of a fluid’s resistance to flow.
(How thick a fluid is.)
4. Elasticity
d. A measure of how easily a solid will
shatter.
4. g/mL
D. Measure of how hard it is to break
something by pulling.
5. Malleability
e. A measure of how easily a solid can be
scratched.
5. ÷
E. Unit of density.
A. A unit of volume that equals 1 mL.
B. In a formula, what the horizontal line
means: ex. the line in: m
v
When building a bridge, engineers want the bridge cables
to have great _________________.
A soccer ball and a
bowling ball are
approximately the
same size.
Glass can be scratched by quartz. Which one is harder?
Lead feels very heavy for its size. It is very __________.
Transmission fluid is a very thick oil that flows slowly.
Transmission fluid is very _____________.
Which one is denser?
Why?
Object A
Which object is the
most dense?
Why?
50 g
When a fluid gets hotter, do you think it will be more or
less viscous? (Think of warmed-up syrup.)
Object B
When gold is hammered it “squishes”. Iron Pyrite is
known as “Fool’s Gold”. It is not ___________ like gold,
but shatter into many pieces when struck by a
hammer. Iron Pyrite is __________.
50 g
A hunter’s wood bow stores energy that is given to the
arrow. The wood’s ability to springs back means it is
very ___________.
An object has a volume of 3.5 cm3 and a mass of
7 grams. Find the object’s density.
Challenge: If a substance has a density of 2.5 g/cm3,
how much mass will 50 cm3 of it have?
If 60 grams of a liquid takes up 120 mL, how dense
is the liquid?
In science we describe substances and their various properties. Each substance has many different properties.
Fill in the following table, deciding how each property best describes the following substances.
Substance
Dense?
Brittle?
Viscous?
Malleable?
Elastic?
Hard?
Tensile
Strength?
Glass
medium
yes
N/A
no
no
yes
high
Rubber
Ice
Molasses
Steel
Styrofoam
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Period: _____________________
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Name: _____________________
Unit 2:2
Period: _____________________
Measuring Density
Mass in grams (g)
The density of an object
is defined as how
compact it is. To find
an object’s density, you
must measure its mass
and volume.
Density:
in g/mL or
g/cm3
Measuring the mass of a solid
is simple with a balance scale.
D= m
v
Volume in
cm3 or mL
Density = Mass ÷ Volume
You can’t measure a liquid by putting it on a scale.
You must measure it while it is inside a container.
Mass of a Liquid
The beaker has more mass afterwards,
since it has a liquid in it.
Mass with liquid − Mass empty = Mass of liquid
450g − 300 g = 150 g
Before (empty)
mempty = 300 g
After (with liquid)
mwith fluid = 450 g
Displacement Method
The liquid has a mass of 150 g.
The displacement method allows you to easily and quickly measure the mass
of an object by measuring how much water it displaces.
The water went up because
the object displaced the water.
30
30
20
20
10
10
Volume after − Volume before = Volume of object
26 mL − 16 mL = 10 mL
The object has a volume of 10 mL.
Before
(Just water)
Vbefore = 16 mL
Floating Objects
The object
floats, so you
can’t find its
volume easily.
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After
(With object)
Vafter = 26 mL
Use the displacement method when an object is hard to
measure because it has a strange or irregular shape.
OR use the displacement method for regular objects just
because it is easy and fast.
If an object floats, it is necessary to submerge it, push it into the water in order to
use the displacement method to find its volume.
Push the object into
the water until the
top of it is at the top
of the water
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Sinking an object—
If an object is hollow and has
a water tight lid you could fill
it with a denser object and
sink it. Be sure to take the
mass of the empty container to
find its density, though.
Copyright © 2006, C. Stephen Murray
Name: _____________________
Unit 2:2
Period: _____________________
How do you measure the mass of a solid?
How do you measure an irregular shaped object?
How do you measure the mass of a liquid?
How do you measure the volume of a floating object?
15
15
15
15
10
10
10
10
5
5
5
5
Volume before: ________
Empty mass: 65 grams
Volume after: ________
Mass with liquid: 88 grams
Volume of liquid: _______
Volume of the toy car: ______________
Mass of the just the liquid: ___________________________
If the mass of the toy car is 14 grams, find its density.
What is the density of the liquid?
The two liquids have the same: ______________
Which one has more mass? _________________
15
15
15
Volume of A: ______ Mass of A: ___________
10
10
10
5
5
5
Density of Liquid A: ______________________
Volume of B: ______ Mass of B: ___________
Density of Liquid B: ______________________
Empty mass:
65 grams
15
10
5
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With Liquid A:
73 grams
Empty mass:
20 grams
With water:
31 grams
15
With liquid B:
71 grams
Find the density
of the liquid in
the cylinder.
15
What is the
volume of
the object?
15
10
10
10
5
5
5
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Name: _____________________
Period: _____________________
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Name: _____________________
Unit 2:3
Period: _____________________
More Density
Less Dense Objects Float
If two objects are put together, the less dense one will float.
Heavy things don’t sink
(unless they are denser).
Light things don’t float
(unless they are less dense).
A ship is heavy, but it floats in
water because it is less dense.
A penny is light, but it sinks in
water because it is more dense.
You can tell by the numbers, too. If the object’s density < Liquid’s density, the object will float.
Ex. 1
Object A: D = 1.56 g/mL
Liquid B: D = 1.2 g/mL
The object sinks! (It is more dense.)
Gases: high energy; low density.
Molecules bounce around,
spreading out.
Gases
More Dense
More Energy
Object A: D = 0.85 g/mL
Liquid B: D = 1.0 g/mL
The object floats! (It is less dense.)
For the same substance the three states of matter
have different energies and different densities.
States of Matter and Density
Liquids
Ex. 2
Liquid
wax
Liquids: Medium energy; medium
density. Molecules slide around,
staying close together.
Solids: Low energy; high density.
Molecules are stuck together.
Solids
Density of Water = 1 g/mL
This means that every mL of water = 1 g
OR every gram of water = 1 mL
This makes calculations
with water easy.
Solids sink in their liquids.
Solid
wax
Solids are denser
than their liquids.
Density of Ice = 0.92 g/mL
Water: The Exception
Solid water floats
in liquid water.
Ice is less dense than water.
Water is the ONLY substance
whose solid floats in its liquid.
Ice
D = 0.92 g/mL
Floating Ice is Important for Life
Water
D = 1 g/mL
Floating ice on lakes and ponds
insulates fish during cold winters.
Vwater (in mL) = mwater (in g)
The expansion of water freezing
breaks down rocks into soil.
Ex. 35 g water = 35 mL
46 mL of water = 46 g
Density Columns
When different liquids are put
together in a column they
separate due to their different
densities. If they are put in a
different order, they will still
end up in the right order.
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Least Dense
By putting an object into the
column you can estimate its density
by where it floats or sinks.
A
Liquid B is more
dense than Liquid A.
Liquid C is more
dense than Liquid B.
B
Most Dense
C
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This object has a density
greater than liquid B, but
less than liquid C.
Copyright © 2006, C. Stephen Murray
Name: _____________________
Unit 2:3
Period: _____________________
1. Solids
A. Only solid that floats in its liquid.
2. 1.0 g/mL
B. Tightly packed atoms; very dense.
3. Gases
C. Loose atoms; low density.
4. 0.92 g/mL
D. Density of water.
5. Density Column
E. Separates liquids by density.
6. Liquids
F. Density of ice.
7. Ice
G. Close atoms; medium density.
True or False? If false, correct the statement.
Light things float.
Heavy things sink.
Circle the one that is more dense.
Sinks or Floats in Water?
__ D = 1.2 g/mL
__ Ice
__ D = 0.85 g/mL
Liquid wax or solid wax?
__ Styrofoam
__ A rock
__ D = 2.2 g/mL
Solid water or liquid water?
Liquid iron or solid iron?
Liquid nitrogen or gaseous nitrogen?
Which liquid is the most dense? A, B, or C?
Which liquid is the least dense? A, B, or C?
What is the density of water?
Which liquid is which? A, B, or C?
D = 1.35 g/mL = Liquid ___
D = 0.86 g/mL = Liquid ___
D = 1.00 g/mL = Liquid ___
C
Label the liquid you know.
A
B
If you have 30 grams of water, how
many mL of water do you have?
How many grams is 23 mL of water?
Draw where ice will float in the column.
How many grams of water is in the
graduated cylinder?
Mass of Liquid A: ________________
Volume of Liquid A: ______________
15
15
15
10
10
10
5
5
5
Density of Liquid A: ______________
Mass of Liquid B: ________________
Volume of Liquid B: ______________
Density of Liquid B: ______________
Empty: 12 grams
With Liquid A: 24 grams
With Liquid B: 28 grams
Which one would float on top?
In the Lab
Mass of empty cylinder:
Fill in the following table for the liquids you are given.
Liquid
Mass
Volume
Density
List the solid objects
you have been given
from least dense to
most dense (guessing).
In what order do you think the liquids will stack?
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Your Final Density Column
Copyright © 2006, C. Stephen Murray
Name: _____________________
Period: _____________________
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Copyright © 2006, C. Stephen Murray
Name: _____________________
Unit 2:4
Period: _____________________
Buoyancy and Archimedes’ Principle
Buoyancy—the upward force of a fluid on an object.
When an object is put into a fluid, it feels lighter
because the fluid pushes up on the object. This is
known as the buoyant force.
A warning buoy is
buoyant (it floats).
60 g
100 g
A denser liquid (usually more viscous) will give more
buoyant force.
A more buoyant object floats better.
A less dense object is more buoyant.
Buoyant force = weight not in fluid – weight in fluid
The mass seems lighter in the liquid.
The liquid pushes up on the mass,
giving buoyant force.
Ex. A 35 Newton object seems to weigh 30 Newtons in water.
35 N – 30 N = 5 Newtons (the buoyant force given by the water)
In order for something to float it must
displace enough fluid to equal its weight.
Archimedes Principle
Noah’s Ark floated
because of
Archimedes’ Principle.
A ship floats because of its shape. With
air in the middle of the ship it displaces
(pushes away) enough water to equal
its mass. A 12 ton ship must displace
at least 12 tons of water to float.
Steel block
1.
2.
Air
A 60 g object seems to be only 40 g when
put into a liquid. How much buoyancy did
the liquid give?
A 150 g object seems to be only 110 g when
put into a liquid. How much buoyancy did
the liquid give?
3.
If an object displaces 20 mL of water.
What is the mass of the displaced water?
4.
If an object has 76 grams of mass,
how much water must it displace to float?
5.
A 125 gram object displaces 100 grams of water.
Will it sink or float?
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Ex 1. A 50 gram object displaces
50 grams of water (50 mL).
It will float.
Steel ship;
Same mass
Less volume
higher density.
It will sink.
Remember:
Same mass
More volume
Less dense, so
it will float!
Ex 2. A 65 gram object displaces
64 grams of water (64 mL).
It will sink.
6.
A 30 gram object displaces 40 grams of water.
Will it sink or float?
7.
A 97 gram object displaces 98 grams of water.
Will it sink or float?
One step farther...
8.
A 60 gram ship displaces 90 grams of water.
How much cargo can it hold before it sinks?
9.
A 85 gram ship displaces 80 grams of water.
How much cargo can it hold before it sinks?
10. A 300 gram ship displaces 800 grams of water.
How much cargo can it hold before it sinks?
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Copyright © 2006, C. Stephen Murray
Name: _____________________
Unit 2:4
Period: _____________________
Buoyancy Lab—Archimedes’ Principle
1) Find the initial mass of the balloon system (balloon with 20 pennies and the binder clip). Record in data table below.
2) How much water will have to be displaced for the balloon system to float? Record below.
3) Level the overflow tank this way:
From the large beaker pour water into the displacement tank until it pours out into the small beaker.
When the water stops flowing into the small beaker, empty the small beaker into the large beaker.
4) Seal the uninflated balloon system with the clip. Put it into the displacement tank and let the water flow into the small beaker.
5) With the graduated cylinder, determine how much water mass the balloon system displaced. Record below.
6) Did the balloon system float or sink? Record below.
7) Retrieve the balloon system. Relevel the overflow tank as in procedure 3).
8) Inflate the balloon just smaller than a tennis ball; seal with the clip; find the water mass displaced. Record below.
9) Relevel the overflow tank as in procedure 3).
10) Inflate the balloon to the size of a baseball (but smaller than the displacement tank). Record the water mass displaced:
QUESTION: Archimedes’ Principle states that the balloon will float if the water it displaces equals the mass of the object.
Did this happen? Record below.
11) Find the volume of the film canister. Record below.
12) Using Archimedes’ Principle determine what the maximum mass the canister can hold and still float. Record below.
13) Measure the mass of one penny: Record below.
14) Predict how many pennies will float in the canister? Record below.
15) Test your hypothesis. Record your data below.
DATA TABLE
1)
Mass of balloons and pennies
2)
Volume of water needed to hold up balloon and pennies
5)
First amount of water displaced
6)
Float or sink?
8)
Second amount of water displaced
10)
Third amount of water displaced
Q:
Archimedes' Principle
11)
Film canister volume
12)
Maximum mass before the canister sinks.
13)
Mass of one penny
14)
Prediction of how many pennies will float.
15)
Maximum # of pennies before it sank.
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Name: _____________________
Period: _____________________
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Period: _____________________
The Atom
Unit 2:5
Atoms, Elements, Molecules, and Compounds
Our modern model of the atom comes from the contributions of several scientist over millennia.
1. The Greek scientist Democritus (BC 460-370)
proposed that there had to be a smallest part of
matter, which he called atomos (indivisible).
negative
electrons
Central
nucleus
Democritus: Indivisible atoms
are hard spheres.
4. The nucleus was discovered in 1911 when
Ernest Rutherford shot alpha particles at gold
foil. Most of the particles passed thru the foil,
since the atom is mostly empty space with a
solid, central nucleus.
Dalton: Each element’s atoms
are the same.
2.
In 1808 John Dalton published a theory of
the atom that had these important points:
5. In 1913 Niels Bohr, while studying light, realized
that electrons can only exist in certain energy levels
or orbitals.
• All atoms of a particular element are the same.
• Atoms of different elements have different
properties, mass, and chemical reactivity.
• Atoms are not changed by chemical reactions,
just rearranged in order or number.
–
+ – +
+
–
– +
Rutherford: the
atom is mostly
empty space
with a solid
nucleus.
negative electrons
electron orbitals
(energy levels).
Electrons cannot
exist between
levels.
nucleus:
contains
positive
protons
and neutral
neutrons
Thomson: plum pudding atom:
negative plums (electrons) in
the positive pudding (atom).
3. Electrons were discovered by J.J. Thomson
in 1897. By watching streams of particles bend
toward positive plates, he realized the particles
were negative. Knowing atoms were neutral, he
thought that electrons were like negative plums
in positive pudding.
Niels Bohr model of the atom.
6. Scientists have now split the atom and even
split protons, neutrons, and electrons into even
smaller particles called quarks.
Subatomic Particles
Particle
Charge
Location
Mass
Tells the
Subatomic means
“smaller than the atom”.
Each particle has different
properties and locations.
proton
positive
Nucleus
1 amu
element
neutron
neutral
Nucleus
1 amu
isotope
electron
negative
Orbitals
1/2000 amu
ion
Atoms, Elements, Molecules, and Compounds
Atoms
Elements
Molecules
Compounds
An atom is a single
piece of an element
that retains the
element’s properties.
An element has only
one kind of atom. All
elements are found on the
periodic table of elements.
A molecule is any
combination of two or
more atoms. Not all
molecules are compound.
A compound is any
combination of two or more
different atoms. All
compounds are molecules.
O
Mg
Cl
Cl
3 atoms
2 elements
1 molecule
1 compound
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He
He
C
4 atoms
3 elements
1 molecule
1 compound
H
O
O
2 atoms
1 element
1 molecule
0 compounds
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H
O
3 atoms
2 elements
1 molecule
1 compound
Copyright © 2006, C. Stephen Murray
Name: _____________________
Unit 2:5
Period: _____________________
1.
2.
3.
Proton.
A. Particles with no charge found in the
nucleus of atoms.
1.
Dalton
Neutron
B. Center of the atom; contains protons
and neutrons.
2.
Bohr
3.
Democritus
C. Realized that there was a smallest part
of matter.
4.
Rutherford
D. Discovered that electrons are in distinct
orbits.
5.
D. The smallest part of an element or
molecule. Building block of all things.
Thompson
E. Theorized that atoms cannot be
changed chemically.
C. Positively charged particle in the
nucleus of the atom. Determines the
element.
Electron
4.
Nucleus
5.
Atom
1.
Molecule
A. Smallest part of an element. Can
only be split by nuclear means.
2.
Compound
B. Any combination of two or more
elements.
3.
Atom
C. Any combination of two or more
atoms, whether the same or different.
4.
Element
D. A substance in which all the atoms
are the same.
A. Discovered that atoms have a nucleus.
B. Discovered the electron.
Draw a picture of an atom, using the Bohr model. Be sure to
label the nucleus, protons, neutrons, electrons, and orbitals.
E. Negative particles in orbits around the
atom.
How did the Rutherford experiment prove the existence of
the nucleus?
Name the subatomic particles that make up the atom.
The number of protons tells you the ________________ .
The number of electrons tells you the _______________ .
The number of neutrons tells you the _______________ .
Atomic #
(number of
protons)
Find the atomic number of:
A) Fe: _______
B) K: _______
C) Ni: _______
D) Al: _______
20
Ca
Find the elements:
A) 8 protons: ________
B) 6 protons: ________
C) 15 protons: ________
D)86 protons: ________
40.078
Give the charges for the following:
1 electron (e): _________
2 electrons (2 e) : ______
2 p + 2 e: _____________
3 p + 3 n + 2 e: ________
1 proton (p): __________
4 protons (4 p): ________
4 p + 2 n: ____________
6 p + 7 n + 8 e: ________
1 neutron (n): _________
3 neutrons (3 n): _______
1 n + 3 p: ____________
9 p + 10 n + 10 e: ______
Li
S
C
F
O
N
O
Li
Atoms:
Elements:
Molecules:
Compounds:
___
___
___
___
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Atoms: ____
Elements: ____
Molecules: ____
Compounds: ___
O
K
H
F
O
O
Li
Atoms: ____
Elements: ____
Molecules: ____
Compounds: ___
Atoms: ____
Elements: ____
Molecules: ____
Compounds: ____
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Atoms:
Elements:
Molecules:
Compounds:
____
____
____
____
Copyright © 2006, C. Stephen Murray
Name: _____________________
Period: _____________________
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Name: _____________________
Unit 2:6
Period: _____________________
Isotopes and Making Atoms
An isotope is a variation of an element. It has the same number of protons
(same element), but a different number of neutrons (different isotope).
Isotopes
Protons
Isotopes of Hydrogen
Because they each have
1 proton, they are all
hydrogen atoms, but are
different isotopes
because they have
numbers of neutrons .
Hydrogen 1
1p + 0n = 1
Isotopes of Beryllium
Neutrons
Hydrogen 2
1p + 1n = 2
Hydrogen 3
1p + 2n = 3
Reading the Tiles
Atomic mass
(average of all the isotopes)
Mass numbers
(Most common isotopes)
Beryllium 8
4p + 4n = 8
Beryllium 9
4p + 5n = 9
Hydrogen
1
Neutrons = mass # – protons
H
For Hydrogen 3:
3 (mass #) – 1 (atomic #) = 2 (neutrons)
1.01
1, 2, 3
Hydrogen 3 has 2 neutrons.
Ions
Neutral Atoms
11p
12n
1 proton = Hydrogen
1 proton (+1)
1 electrons (–1)
+1 –1 = 0
neutral atom
Mass # = protons + neutrons
If the number of electrons equals the number of
protons the atom is neutral. If not, it is an ion.
Ions and Neutral Atoms
2 protons = Helium
2 proton (+2)
2 electrons (–2)
+2 –2 = 0
neutral atom
attract
8p
8n
Positive and
negative
ions attract
each other.
8 protons = Oxygen
8 p –10e = –2
negative ion: O –2
11 protons = Sodium
11 p –10e = +1
positive ion: Na+1
Electrons will want fill up inner orbits first to get as close to the nucleus as possible.
They also want to stay as far away from each other as possible.
Electrons Orbits
–
Like charges
repel
–
–
electron
2 electrons
Opposites
attract
+
4p
5n
Finding the # of Neutrons
Atomic number
(number of protons)
The atomic mass
is an average.
Round it to
find the most
common isotope.
4p
4n
proton
lithium
lithium
The # of elements
in a row = # of
electrons in a level.
# rows = # of
energy levels.
End of a row
means a full
energy level.
1st level
2nd level
3rd level
3p
3n
3p
3n
Incorrect! - The electrons will
fill up the inner levels first.
The first level takes 2 electrons.
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Correct! - Inner orbit
is full (with 2);
one outer electron.
4th level
Sodium starts the
3rd electron levels.
Neon has 2 filled
energy levels.
1st row has 2 elements, so the first
energy level can hold 2 electrons.
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Copyright © 2006, C. Stephen Murray
Name: _____________________
Unit 2:6
Period: _____________________
1. Isotope
A. An average of all the isotopes; the
mass of average atom.
2. Atomic mass
B. An atom with an equal number of
electrons and protons.
Give abbreviations and number of protons
Calcium (Ca)
3. Atomic #
C. An atom with more or less electrons
than protons.
4. Neutral atom
D. A variation of an element with a
different number of neutrons.
5. Ion
E. Total number of protons and neutrons
in the nucleus.
6. Mass #
F. Number of protons; determines the
element.
7 protons and 10 electrons.
15 protons and 15 electrons.
35 protons and 37 electrons.
89 protons and 89 electrons.
Neutral atom or ion?
Neutral atom or ion?
Neutral atom or ion?
Neutral atom or ion?
Give the element abbreviation and charge.
5 protons and 2 electrons: Element: B Charge:
.
Boron (____) __________
Potassium (____)________
Selenium (____) _______
Copper (____) __________
Silver (____)___________
Zirconium (____) _______
Mercury (____) ________
20
Which of the following are isotopes?
Element A: 15 protons; 15 electrons; 16 neutrons
Element B: 14 protons; 16 electrons; 14 neutrons
Element C: 15 protons; 18 electrons; 15 neutrons
Element D: 16 protons; 18 electrons; 15 neutrons
Element E: 15 protons; 18 electrons; 14 neutrons
Sulfur 32 has 16 protons and 16 neutrons. (32 – 16p = 16n)
Magnesium 25 has ___ protons and _________ neutrons.
Carbon 14 has ___ protons and _________ neutrons.
+3
.
Lithium 7 has ___ protons and _________ neutrons.
16 protons and 18 electrons: Element:
Charge:
.
35 protons and 36 electrons: Element:
Charge:
.
Chlorine 35 has ___ protons and _________ neutrons.
12 protons and 10 electrons: Element:
Charge:
.
Fluorine 19 has ___ protons and _________ neutrons.
What’s wrong with this
picture of an atom?
neutron
Oxygen 16 has how many neutrons?
proton
Beryllium 8 has how many neutrons?
electron
This picture is supposed to
be of a neutral atom. Fix it.
Boron 11 has how many neutrons?
Which row is Lithium (Li) in? 2 . It has electrons in levels
1 and 2.
10p
11n
Which row is phosphorous (___) in? ____ So, phosphorous
has electrons in which electron levels?
Which row is calcium (___) in? ____ So, calcium has
electrons in what levels?
What is wrong with this
picture of an atom?
Which row is argon (___) in? ____ So, argon has electrons
in what levels?
8p
7n
Argon (___) is at the end of row ___. So argon has ____
full electron levels.
Helium (___) is at the end of row ___. So helium has ____
full electron levels.
What is wrong with this
picture of an atom?
Xenon (___) is at the end of row ___. So xenon has ____
full electron levels.
7p
7n
How many full electron levels does Calcium have?
How many full electron levels does Sulfur have?
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Name: _____________________
Period: _____________________
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Name: _____________________
Unit 2:7
Period: _____________________
Metals, Non-Metals and Valence Electrons
Valence Electrons are the outermost electrons in an atom.
Each group (column) has the same number of valence electrons.
Only valence electrons are involved in chemical bonding.
Valence Electrons
Lithium 6
Hydrogen 1
Oxygen 17
3p
3n
1p
Inner electrons
are NOT
valence electrons
8p
9n
1 valence electron
1 valence electron
Hydrogen and Lithium are both in
Group 1A—both have 1 valence electrons.
6 valence electrons
Octet Rule – Atom are
more stable that have a full
shell of electrons. For most
atoms 8 valence electrons is
full (octed = 8). For H and
He this number is 2. Atoms
want to have 8 valence
electrons. “If I 8, I full.”
Only elements in Group
18A have a full octet
(8 valence electrons)
naturally. All other
elements will lose, gain,
or share to reach 8 electrons.
Elements with the same valence electrons have
similar reactivity, so they tend to react the same.
Valence Electrons
1
8
1A
18A
2
1
H
2A
Electron
Levels 2
(Periods)
3
Li
4
Be
3
11
Na
12
Mg
4
19
K
20
Ca
1
2
1
Groups
Groups
Divides
metals and
non-metals
Transition Metals
(valence electrons vary)
Metals
3
4
5
6
7
13A
14A
15A
16A
17A
2
He
5
B
6
C
7
N
8
O
9
F
10
Ne
13
Al
14
Si
15
P
16
S
17
Cl
18
Ar
31
Ga
32
Ge
33
As
34
Se
35
Br
36
Kr
3
4
5
6
7
8
Non-metals
Metals and Nonmetals
Metals or Non-metal?
Metals are on the left side of the periodic
table. Non-metals are on the right side.
Metals and non-metals have different
properties and bond differently,
making different kinds of compounds.
Calcium (Ca): metal (left side)
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Exception:
Helium
only has 2
valence
electrons!
Going Farther
Bromine (Br): non-metal (right side)
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Along the separation line are
the semimetals or metalloids:
Boron (B), Silicon (Si),
Germanium (Ge), Arsenic
(As), Antimony (Sb). These
have properties of both
metals and non-metals.
Copyright © 2006, C. Stephen Murray
Name: _____________________
Unit 2:7
Period: _____________________
1. Octet Rule
A. Elements found on the right side of
the periodic table.
How many valence electrons?
2. Metals
B. Elements found on the left side of the
periodic table.
Calcium (Ca)
.
Hydrogen (____) _______
Potassium (____)________
Helium (____) _________
3. Valence
electrons
C. Says that atoms tend to be more stable
with eight valence electrons.
Oxygen (____) _________
Aluminum(____) _______
Argon (____) __________
Sodium (____) _________
4. Non-metals
D. Electrons in the outermost electron
level. Involved in chemical bonding.
Boron (____) ___________
Nitrogen (____) ________
Metal or Non-metal?
Connect the element on the left with the element
on the right that has similar reactivity.
__M__ Aluminum ( Al )
____ Iron (___)
____ Oxygen (___)
____ Fluorine (___)
____ Gold (___)
____ Tin (___)
____ Nitrogen (___)
____ Lithium (___)
____ Bromine (___)
____ Chromium (___)
____ Krypton (___)
____ Lead (___)
Chlorine
Phosphorous
Magnesium
Sodium
Boron
Sulfur
+3
.
Charge:
.
35 protons and 36 electrons: Element:
Charge:
.
2p
2n
10p
11n
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Elements with the
same # of
__________
__________ have
the same reactivity.
Are these elements isotopes of one another?
Element A: 14 protons; 15 electrons; 13 neutrons.
Element B: 14 protons; 14 electrons; 15 neutrons.
16 protons and 18 electrons: Element:
11p
12n
Beryllium
Potassium
Iodine
Aluminum
Oxygen
Nitrogen
Are these elements isotopes of one another?
Element A: 12 protons; 11 electrons; 13 neutrons.
Element B: 13 protons; 12 electrons; 13 neutrons.
7 protons and 10 electrons. Neutral atom or ion?
15 protons and 15 electrons. Neutral atom or ion?
35 protons and 37 electrons. Neutral atom or ion?
Give the element abbreviation and charge.
5 protons and 2 electrons: Element: B Charge:
2
Element: _______________
# of neutrons: ___________
Mass #: ________________
# of electrons: ___________
# of valence electrons: ____
It is an ion? _____________
Are these elements isotopes of one another?
Element A: 12 protons; 11 electrons; 13 neutrons.
Element B: 12 protons; 12 electrons; 13 neutrons.
Are these elements isotopes of one another?
Element A: 18 protons; 18 electrons; 18 neutrons.
Element B: 18 protons; 18 electrons; 19 neutrons.
Sulfur (_S_) is in row __3__. Sulfur has __2___ complete
electron levels and __6_ valence electrons in level __3___.
Element: _______________
# of neutrons: ___________
Mass #: ________________
# of electrons: ___________
# of valence electrons: ____
It is an ion? _____________
Magnesium (____) is in row ____. Magnesium has _____
complete electron levels and _____ valence electrons in
Element: _______________
# of neutrons: ___________
Mass #: ________________
# of electrons: ___________
# of valence electrons: ____
It is an ion? _____________
Potassium (___) is in row ____. Potassium has ____
complete electron levels and _____ valence electrons in
level _____.
Carbon (____) is in row ____. Carbon has _____ complete
electron levels and _____ valence electrons in level _____.
level _____.
Argon (____) is in row ____. Argon has _____ complete
electron levels and _____ valence electrons in level _____.
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Name: _____________________
Period: _____________________
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Name: _____________________
Unit 2:8
Properties of Matter Review
Period: _____________________
1. Density
a. A measure of how easily a solid can be
scratched.
1.Tensile
Strength
2. Brittleness
b. A measurement of how easily a solid
can be pounded into thin sheets.
2. viscosity
A. A unit of volume that equals 1 mL.
B. Measure of a fluid’s resistance to flow.
(How thick a fluid is.)
C. Measure of how hard it is to break
3
c. A measurement of the “compactness” of 3. cm
something by pulling.
a substance; ratio of mass to volume.
D. Unit of density.
4. 5. ÷
d. Measure of a solid’s ability to return to
its original shape after stretching.
E. In a formula, what the horizontal line
5. g/mL
means: ex. the line in:
e. A measure of how easily a solid will
shatter.
A rock climber wants a rope with great ________________.
3. Hardness
4. Elasticity
5. Malleability
Object A
Which object is the
less dense?
Why?
50 g
Object B
50 g
An airplane pilot wants a windshield that is ___________.
A child bends a toy. It stays bent because it wasn’t very
__________.
I step on a ball of aluminum foil. The aluminum flattens
because it is very ______________.
Which object is the
less dense?
Object A
Object B
In Alaska, cars need oil that is thinner and flows faster, so
during the cold winter it doesn’t become too ___________.
Why?
50 g
80 g
A 15 g object has a volume of 30 cm3. Find its density.
Balsa wood is very light for its size, so it is not very _______.
We give small children plastic dishes because ceramic dishes
are too _________ and break too easily
A piece of wood floats because it has ______________.
A 12 g object has a volume of 6 mL. Find its density.
How do you measure the mass of a liquid?
How do you measure the volume of a floating object?
A 35 mL object has a density of 2 g/mL. Find its mass.
Which is more dense: liquid iron or solid iron?
Which is more dense: gaseous CO2 or liquid CO2?
Which is more dense: liquid water or solid water?
A 200 g object displaces 150 g of water. Float or sink?
A 300 g object displaces 350 g of water. Float or sink?
15
15
12 grams
10
5
A 250 g object displaces 300 g of water. How much cargo
can it hold?
10
5
C
B
What is the volume of the object?
What is the object’s density?
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A
Which liquid is which? A, B, or C?
D = 1.00 g/mL = Liquid ___
D = 0.75 g/mL = Liquid ___
D = 1.83 g/mL = Liquid ___
Label the liquid you know.
Draw where ice will be in the column.
In the column, where would a cube of
density 0.89 be?
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Copyright © 2006, C. Stephen Murray
Name: _____________________
Unit 2:8
Period: _____________________
1. Isotope
A. An average of all the isotopes; the
mass of average atom.
How many valence electrons?
2. Atomic mass
B. An atom with an equal number of
electrons and protons.
Helium (____) _________
Lithium (____) _________
Calcium (____) _________
Aluminum (____) _______
3. Atomic #
C. An atom with more or less electrons
than protons.
Sulfur (____) __________
Nitrogen (____) _________
4. Neutral atom
D. A variation of an element with a
different number of neutrons.
5. Ion
E. Total number of protons and neutrons
in the nucleus.
6. Mass #
F. Number of protons; determines the
element.
Calcium and ___________ have the same reactivity.
Oxygen and ___________ have the same reactivity.
Helium and ___________ have the same reactivity.
1.
Bohr
A. Discovered that atoms have a nucleus.
2.
Dalton
B. Realized that there was a smallest part
of matter.
3.
Democritus
C. Discovered that electrons are in distinct
orbits.
Metal or Non-metal?
____ Titanium (___)
____ Neon (___)
____ Sodium (___)
____ Hydrogen (___)
4.
Rutherford
D. Discovered the electron.
____ Chlorine (___)
____ Nickel (___)
5.
Thompson
E. Theorized that atoms cannot be
changed chemically.
8 protons and 10 electrons. Neutral atom or ion?
16 protons and 18 electrons. Neutral atom or ion?
20 protons and electrons.
Neutral atom or ion?
A 35 N object feels like 30 N when lowered into a liquid.
How much b______ force does the liquid give?
Give the element abbreviation and charge.
16 protons and 18 electrons: Element:
Charge:
.
35 protons and 36 electrons: Element:
.
Charge:
Nitrogen with 10 electrons. Charge: _________.
If put into a more v_______ liquid, the object would feel
even lighter.
“Atoms are solid.” Respond and give reasons for your
response.
Be
For all of the above:
Atoms: _______
Elements: _______
Molecules: _______
Compounds: _______
Are these different elements?
Element A: 17 protons; 18 electrons; 16 neutrons.
Element B: 18 protons; 18 electrons; 18 neutrons.
Why?
What is wrong with this
picture of an atom?
8p
7n
Are these different isotopes of one another?
Element A: 12 protons; 11 electrons; 13 neutrons.
Element B: 12 protons; 12 electrons; 14 neutrons.
Why?
Are these different isotopes of one another?
Element A: 18 protons; 18 electrons; 18 neutrons.
Element B: 19 protons; 18 electrons; 19 neutrons.
Why?
12p
13n
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Element: _______________
# of neutrons: ___________
Mass #: ________________
# of electrons: ___________
# of valence electrons: _____
It is an ion? _____________
Calcium (___) is in row ____. Calcium has _____ complete
electron levels and _____ valence electrons in level _____.
Sulfur (____) is in row ____. Argon has _____ complete
electron levels and _____ valence electrons in level _____.
Legal copying of this worksheet requires written permission.
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Name: _____________________
Period: _____________________
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Name: _____________________
Period: _____________________
Electrons are not as close
to protons as possible
(should fill in inner
levels first
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Name: _____________________
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IPC Lab – 1st Sixth Week—Density Column Lab
In this Investigation you will:
- Find the density of various liquids.
- Approximate viscosity of various liquids.
- Make a density column of liquids.
- Use the density column to approximate the density of solids.
Lab Safety:
Goggles: to protect your eyes from the various liquids.
Apron: to protect your clothes.
Pre-Lab Review (Answer these 5 questions first):
What two measurements do we need to find density?
What is the equation for density?
If the density of a solid is less than the density of a liquid will it:
sink or float? (pick one)
If the density of a solid is more than the density of a liquid will it:
sink or float? (pick one)
A liquid of greater viscosity will flow slower or faster?
Procedure 1: Measuring the Density of the Five Liquids
Find the mass of the 10 mL plastic graduated cylinder and record in the table.
Using the plastic cylinder find the mass and volume of each of the five liquids and
record in the table.
Remember to rinse the graduated cylinder between each liquid.
Calculate the density of each liquid.
Fluid
Green Corn Syrup
Mass of Fluid and
Cylinder
Mass of Cylinder
Mass of Fluid
Volume of
Fluid
Density of
Fluid
Blue Dish Soap
Red Water
Clear Cooking Oil
Gold Honey
Procedure 2: Predicting How to Stack the Liquids
Using the densities that you calculated in Procedure 1 determine the order you will place the liquids in the 100 mL
cylinder.
In the following table, write your prediction of how the liquids should be stacked.
Liquid 5 (top)
Liquid 4
Liquid 3
Liquid 2
Liquid 1 (bottom)
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Name: _____________________
Period: _____________________
Procedure 3: Constructing Your Density Column
You will construct your density column in the 100 mL graduated cylinder. You will use the
remainder of the five fluids.
Slowly pour your predicted Liquid 1 into the cylinder.
Pour each of the remaining liquid in to the graduated cylinder in the order of the previous table.
Be sure to remember how fast each liquid pours into the cylinder.
Was your predicted density order correct? __________.
If not, what happened? __________________________________________________.
Use the flowing speed to determine the order of viscosity of the five fluids:
Greatest viscosity
Least viscosity
Procedure 4: Comparing the Density of Solids
A solid placed in a liquid will float if it is less dense and sink if it is more dense.
Predict where the following six objects (penny; cork; crayon; dice; ice; aluminum foil ball)
will float in the density column.
Object 1 (floats on top)
Object 2
Object 3
Object 4
Object 5
Object 6 (sinks to bottom)
Procedure 5: Placing the Solids in the Column
Gently drop each object into the column from most to least dense.
The approximate density of the crayon must be between: _____ g/mL and ____ g/mL
Using the displacement method find the actual density of the crayon:
Mass:
Volume:
Density:
Did your calculation fall within your estimation of the crayon’s density?
Below draw and label the final configuration of your density column (the liquids and where the solids floated).
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Name: _____________________
Period: _____________________
Teacher Explanation Page – (Density Column Lab)
Setup and Preparation:
Use 100 mL graduated cylinders for the density columns.
You will have to color the liquids beforehand. The colors help the students distinguish each
liquid in the column.
You may decide to have each group find the density or only one or two liquids, which can be shared with the entire
class. For each group to find each density is time consuming.
Use 10mL plastic graduated cylinders for students to measure liquid density.
Student Outcome –
Write a scientific statement that explains the relationship between density and placement in the column.
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