Atoms, Elements and Compounds Student Pages:
Chemistry dictionary reference pages0001
Chemistry dictionary reference pages0002
Chemistry dictionary reference pages0003
Chemistry dictionary reference pages0004
Science Experiment Lab Report
Another Chemical Reaction
Ion Gizmo
Subatomic Particle Gizmo
CW Models of Atom Combinations
Elements Matching
Diffusion Experiment0001
Diffusion Experiment0002
Diffusion Experiment0003
Lesson on Naming Compounds
Naming Compounds Worksheet
Chemical Bonding Terms matching quiz
Physical and Chemical Change Worksheet
Models of Acids and Bases0001
Models of Acids and Bases0002
SCIENCE EXPERIMENT WORKSHEET
Name: _______________________________________Grade: ______________________
Project Title: _____________________________________________________________
Statement of the problem (Ask a Testable Question):_____________________________
_________________________________________________________________________
Hypothesis (Prediction: what I think will happen): ________________________________
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Plan the Experiment (Rough Draft): __________________________________________
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Equipment and materials (List the Materials): __________________________________
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Procedure (What I plan to do): _______________________________________________
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Record Data and Observations: _____________________________________________
_________________________________________________________________________
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_________________________________________________________________________
Interpret Data and Observations:
_________________________________________________________________________
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Conclusion (What I found out by doing this experiment): ___________________________
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Apply Findings (How can the results of the experiment be used): ____________________
_________________________________________________________________________
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Attach notes, measurements, photos, tables or graphs to this sheet.
Ion Gizmo
Name _____________________ Pd _____
Electron Dot Diagrams
Before you begin, answer the following questions.
1.
What is a valence electron?
2. How do you determine the total number of electrons in the electron cloud of an atom?
3. How do you determine the number of valence electrons that an atom has?
4. How many total electrons does a carbon atom have?
5. How many valence electrons does a carbon atom have?
I.
Create an atom that contains 4 protons, 5 neutrons and 4 electrons. Check Show electron
dot diagram.
1.
What element is this?
2. What is its atomic number?
3. What is its mass number?
4. What is the net charge of the atom? The net charge can be found in the top left of
the symbol.
II.
Now take away two of the electrons to have an ion with 4 protons, 5 neutrons, and 2
electrons?
1.
What is the charge on a proton?
2. What is the charge on an electron?
3. What is the charge on the ion? (Look at the top right of the element notation)
4. Describe the relationship between the number of protons and electrons in the ion
that was formed when the two electrons were removed.
5. Why did the ion formed have the charge that it received?
III. Create an atom that contains 9 protons, 10 neutrons and 9 electrons.
1.
What element is this?
2. What is its atomic number?
3. What is its mass number?
4. What is the net charge of the atom? The net charge can be found in the top left of
the symbol.
IV.
Now add one electron to have an ion with 9 protons, 10 neutrons, and 10 electrons?
1.
What is the charge on a proton?
2. What is the charge on an electron?
3. What is the charge on the ion? (Look at the top right of the element notation)
4. Describe the relationship between the number of protons and electrons in the ion
that was formed when the electron was added.
5. Why did the ion formed have the charge that it received?
V.
Create a neutral neon atom with 10 protons, 10 neutrons, and 10 electrons?
1.
What is the charge on the atom?
2. Why is the charge neutral?
3. Draw the atom from the gizmo (not the dot structure the “actual” picture of the
atom?
VI.
Create a neutral oxygen atom with 8 protons, 8 neutrons, and 8 electrons.
1.
What is the charge on the atom?
2. Draw the atom from the gizmo.
3. Since the noble gases are stable (VERY unreactive), oxygen would like to look like
one in terms of the number and arrangement of its electrons. What would the atom
of oxygen have to do to its electrons in order to look like neon?
4. Now do this and draw the new ion formed. What is the charge on the ion?
5. Why does the ion have the charge that it does?
6. Since all elements in group 16 have the same number of valence electrons, then they
all behave the same way in order to look like the noble gases. Therefore, what would
an atom in group 16 have to do to look like a noble gas?
VII. Create a neutral fluorine atom with 9 protons, 10 neutrons, and 9 electrons.
1.
What is the charge on the atom?
2. Draw the atom from the gizmo.
3. Since the noble gases are stable (VERY unreactive), fluorine would like to look like
one in terms of the number and arrangement of its electrons. What would the atom
of fluorine have to do to its electrons in order to look like neon?
4. Now do this and draw the new ion formed. What is the charge on the ion?
5. Why does the ion have the charge that it does?
6. Since all elements in group 17 have the same number of valence electrons, then they
all behave the same way in order to look like the noble gases. Therefore, what would
an atom in group 17 have to do to look like a noble gas and what would be the
resulting charge?
VIII.Create a neutral sodium atom with 11 protons, 12 neutrons, and 11 electrons.
1.
What is the charge on the atom?
2. Draw the atom from the gizmo.
3. Since the noble gases are stable (VERY unreactive), sodium would like to look like
one in terms of the number and arrangement of its electrons. What would the atom
of sodium have to do to its electrons in order to look like neon?
4. Now do this and draw the new ion formed. What is the charge on the ion?
5. Why does the ion have the charge that it does?
6. Since all elements in group 1 have the same number of valence electrons, then they
all behave the same way in order to look like the noble gases. Therefore, what would
an atom in group 1 have to do to look like a noble gas and what would be the resulting
charge?
IX.
Create a neutral magnesium atom with 12 protons, 12 neutrons, and 12 electrons.
1.
What is the charge on the atom?
2. Draw the atom from the gizmo.
3. Since the noble gases are stable (VERY unreactive), magnesium would like to look
like one in terms of the number and arrangement of its electrons. What would the
atom of magnesium have to do to its electrons in order to look like neon?
4. Now do this and draw the new ion formed. What is the charge on the ion?
5. Why does the ion have the charge that it does?
6. Since all elements in group 2 have the same number of valence electrons, then they
all behave the same way in order to look like the noble gases. Therefore, what would
an atom in group 2 have to do to look like a noble gas and what would be the resulting
charge?
Subatomic Particle Gizmo (2.1)
_________________________ Pd ___
Name
Some of the greatest breakthroughs in understanding the structure of the atom were provided by
J. J. Thompson during his time at the renowned Cavendish Laboratory in Cambridge, England.
Thompson had a reputation for being rather clumsy with his hands, and he always needed to have
assistants to set up equipment for him. Nevertheless, he was a brilliant experimental physicist.
Work conducted under his watchful eye led to the first discovery of a subatomic particle, the
electron.
Once you log in, find the “Element Builder” Gizmo and select “Launch Gizmo.”
Location of Subatomic Particles
1.
In this Gizmotm, subatomic particles (protons, neutrons and electrons) can be added to an
atom or removed from it by clicking the arrows next to each supply of particles. Remove any
protons (the program will not let you remove the last proton), neutrons, or electrons that
are currently in the atom by clicking the left arrows. You can also highlight the number
with the cursor and change the numbers manually. Below is what the screen should look like
when you begin. The center of the atom is the nucleus and the area around the nucleus is
the electron cloud.
a.
Particle
Using the right arrows, add 1 proton, 2 neutrons, and 2 electrons to the atom so
that there are 2 of each of the three particles located in the atom. Fill in the
following chart.
Location
Proton
Neutron
Electron
Identity of the Atom
2. Place a check in the “Show element name” box, which is in the top right portion of the
gizmo. Manipulate the number of protons to achieve the number of protons in the data
table. Do not worry about the number of neutrons or electrons. Experiment with adding
one and removing one proton to and from the atom. Fill in the following table. Once you have
the identity of the element, look at the periodic table and write down the atomic number
for the element, this is the integer located above the name of the element.
Number of protons
Name of element
Atomic Number from Periodic
Table
2
3
1
a.
Does changing the number of protons change the identity of the element you have
built?
b. What is the relationship between the number of protons and the atomic number for
an element?
3. Now you will do the same thing as step 2 except you will be changing the number of
neutrons. Make sure that you begin with 2 each for the protons, neutrons, and electrons.
Add one neutron to the atom to place 3 neutrons in the atom. Record the name of the
element and look at the periodic table to find the atomic number. Next, take 2 neutrons
away (a total of 1 should now be in the atom.) Again record the name of the atom and the
atomic number from the periodic table.
Number of neutrons
Name of element
Atomic Number from Periodic
Table
2
3
1
a.
Does changing the number of neutrons change the identity of the element you have
built?
b. Does changing the number of neutrons change the affect the atomic number?
4. Make sure that you have 2 each for the protons, neutrons, and electrons. Add one electron
to the atom to place 3 electrons in the atom. Record the name of the element and look at
the periodic table to find the atomic number. Next, take 2 electrons away (a total of 1
should now be in the atom.) Again record the name of the atom and the atomic number from
the periodic table.
Number of electrons
Name of element
Atomic Number from Periodic
Table
2
3
1
a.
Does changing the number of electrons change the identity of the element you have
built?
KEY FACT: Now looking at questions 2a, 3a, and 4a, which subatomic particle is responsible for the
identity of an atom?
Mass of an atom
5. Build an atom again with exactly 2 protons, 2 neutrons, and 2 electrons. Check “Show
element symbol.” Be sure “isotope” is not selected. Make adjustments to the atom to attain
the number of protons, neutrons, and electrons as shown in the data table. Then finish
filling in the table. The number to the upper left of the symbol indicates the mass of
the atom. (See where the pointer is pointing in the screen shot.)
Number of protons Number of
neutrons
2
2
Number of
electrons
2
3
2
2
2
3
2
2
2
3
a.
Identity of atom
(give name)
Mass of atom
Does the proton affect the mass of an atom? You MUST justify your answer.
b. Does the neutron affect the mass of an atom? You MUST justify your answer.
c.
Does the electron affect the mass of an atom? You MUST justify your answer.
d. Looking at the atom in the Gizmo, where is most of the mass of an atom
concentrated? Explain.
5. Which 2 subatomic particles affect the mass of an atom?
KEY FACT: Write a mathematical formula to show the relationship between the number of
protons, the number of neutrons, and the mass number for an atom.
SUMMARY: Based on this gizmo, the number of protons equals the _______________
______________ from the periodic table. The number of protons determines the
_______________ of an atom. The ____________ and _______________ determines the mass
of an atom. The protons and neutrons are located in the ________________ of an atom and
electrons are in the ________________ ______________.
How many protons are in the nucleus of an atom of Carbon (C)?
What is the formula for finding the mass number of an atom?
If an atom of C has 7 neutrons in the nucleus, then it would have a mass number of ______. (see
previous 2 questions)
How many electrons would be found in the nucleus?
Elements: Matching
Use the following words:
_____ H
1)Cobalt
_____ Li
26)Nickel
_____ B
2)Carbon
_____ N
27)Zinc
_____ O
3)Strontium
_____ Ne
28)Aluminum
_____ Na
4)Sulfur
_____ Al
29)Lead
_____ Si
5)Tin
_____ Cl
6)Argon
_____ Fe
7)Boron
_____ Cu
8)Oxygen
_____ Kr
9)Nitrogen
_____ Au
10)Potassium
_____ K
11)Silicon
_____ He
12)Silver
_____ C
13)Gold
_____ F
17)Bromine
_____ Mg
18)Calcium
_____ P
19)Fluorine
_____ Ar
20)Lithium
_____ Co
21)Mercury
_____ Zn
22)Krypton
_____ Sr
23)Helium
_____ Hg
24)Hydrogen
_____ Ag
25)Neon
_____ S
14)Iodine
_____ Ca
15)Phosphorous
_____ Ni
16)Chlorine
_____ Br
30)Copper
_____ Sn
31)Magnesium
_____ Pb
32)Iron
_____ I
33)Sodium
Lesson on Naming Compounds:
Types of Compounds
Ionic compounds are compounds composed of ions, charged particles that form when
an atom (or group of atoms, in the case of polyatomic ions) gains or loses electrons.
•
A cation is a positively charged ion
•
An anion is a negatively charged ion.
Covalent or molecular compounds form when elements share electrons in a covalent
bond to form molecules. Molecular compounds are electrically neutral.
Ionic compounds are (usually) formed when a metal reacts with a nonmetal (or a
polyatomic ion). Covalent compounds are formed when two nonmetals react with each
other. Since hydrogen is a nonmetal, binary compounds containing hydrogen are also
usually covalent compounds.
•
Metal + Nonmetal —> ionic compound (usually)
•
Metal + Polyatomic ion —> ionic compound (usually)
•
Nonmetal + Nonmetal —> covalent compound (usually)
•
Hydrogen + Nonmetal —> covalent compound (usually)
Naming Chemical Compounds – Some Notes
1.
Some nonmetals form a series of polyatomic ions with oxygen (all having the
same charge): ClO-, hypochlorite; ClO2-, chlorite; ClO3-, chlorate; ClO4-,
perchlorate.
a.
The -ate forms (formula and charge) must be memorized. In some cases,
the -ate form has three oxygens, and in some cases four oxygens. The
charge is the same for the entire series.
b.
The -ite form has one less oxygen that the -ate form.
c.
The hypo- stem -ite form has two less oxygens than the -ate form.
d.
The per- stem -ate form has one more oxygen than the -ate form.
e.
The -ide form is the monatomic anion
2.
The cation is written first, followed by the monatomic or polyatomic anion.
3.
The subscripts in the formula must produce an electrically neutral formula unit.
(That is, the total amount of positive charge must equal the total amount of
negative charge.)
4.
The subscripts should be the smallest set of whole numbers possible.
5.
If there is only one of a polyatomic ion in the formula, do not place parentheses
around it; e.g., NaNO3, not Na(NO3). If there is more than one of a polyatomic ion
in the formula, put the ion in parentheses, and place the subscript after the
parentheses; e.g., Ca(OH)2, Ba3(PO4)2, etc.
Remember the Prime Directive in writing formulas:
Ca(OH)2 is not the same as CaOH2 !
Examples
Cation
Na+
Ca2+
Na+
Mg2+
Fe3+
Na+
Anion
ClBrS2O2O2SO42-
Formula
NaCl
CaBr2
Na2S
MgO
Fe2O3
Na2SO4
1. Binary Ionic Compounds Containing a Metal and a Nonmetal.
A binary compound is a compound formed from two different elements. There may or
may not be more than one of each element. A diatomic compound (or diatomic
molecule) contains two atoms, which may or may not be the same.
Metals combine with nonmetals to give ionic compounds. When naming binary ionic
compounds, name the cation first (specifying the charge, if necessary), then the
nonmetal anion (element stem + -ide).
4. Binary Covalent Compounds Between Two Nonmetals.
Two nonmetals combine to form a covalent or molecular compound (i.e., one that is
held together by covalent bonds which result from the sharing of electrons).
In many cases, two elements can combine in several different ways to make completely
different compounds. (This cannot happen with ionic compounds, except in the cases of
metals that can form more than one charge.) For instance, carbon can share electrons
with one oxygen to make CO (carbon monoxide), or with two oxygens to make CO2
(carbon dioxide). For this reason, it is necessary to specify how many of each element
is present within the compound.
•
The formula is written with the more electropositive element (the one
further to the left on the periodic table) placed first, then the more
electronegative element (the one further to the right on the periodic table).
[Important exception: when the compound contains oxygen and a halogen, the halogen
is placed first. If both elements are in the same group, the one with the higher period
number is named first.]
•
The first element in the formula is given the neutral element name, and the
second one is named by replacing the ending of the neutral element name
with -ide. A prefix is used in front of each element name to indicate how
many atoms of that element are present:
1
2
3
4
5
6
7
8
9
10
•
monoditritetrapentahexaheptaoctanonadeca-
If there is only one of the first element in the formula, the mono- prefix is
dropped.
Examples
SO2
SO3
N 2O
NO
NO2
N2O4
N2O5
sulfur dioxide
sulfur trioxide
dinitrogen monoxide
nitrogen monoxide
nitrogen dioxide
dinitrogen tetroxide
dinitrogen pentoxide
Nonmetals may combine in a variety of ratios, so it is important that the name of a
molecular compound indicates how many atoms of each type of element are present in
the compound. This is accomplished using prefixes. If there is only one atom of the first
element, no prefix is used. It is customary to prefix the name of one atom of the second
element with mono-. For example, CO is named carbon monoxide rather than carbon
oxide.
Examples of Covalent Compound Names
SO2 - sulfur dioxide
SF6 - sulfur hexafluoride
CCl4 - carbon tetrachloride
NI3 - nitrogen triiodide
Writing the Formula from the Name
You can write the formula for a covalent compound from its name by writing the symbols
for the first and second element and translating the prefixes into subscripts. For
example, xenon hexafluoride would be written XF6. It is common for students to confuse
ionic compounds and covalent compounds and then have trouble trying to write
formulae from the compounds names. You aren't balancing charges of covalent
compounds; if the compound does not contain a metal, don't try to balance this!
For IONIC Compounds follow these instructions:
Suppose we wish to write the formula for the compound that forms between aluminum
and chlorine. To write the formula, we must first determine the oxidation numbers of the
ions that would be formed. We will revisit the concept of oxidation numbers later, but for
now, all you need to know is that the oxidation number for an atom in an ionic
compound is equal to the charge of the ion it produces.
Then, we determine the simplest whole numbers with which to multiply these charges
so they will balance (add to zero) since ionic compounds are neutral. In this case, we
would multiply the
by and the
by .
You should note that we could multiply the
by and the
by to get
and
,
respectively. These values will also balance, but this is not acceptable because
empirical formulas, by definition, must have the lowest whole number multipliers. Once
we have the lowest whole number multipliers, those multipliers become the subscripts
for the symbols. The formula for this compound would be
.
Here’s the process for writing the formula for the compound formed between aluminum
and sulfur.
Therefore, the formula for this compound would be
.
Another method used to write formulas is called the criss-cross method. It is a quick
method, but it often produces errors if the user doesn’t pay attention to the results. The
example below demonstrates the criss-cross method for writing the formula of a
compound formed from aluminum and oxygen. In the criss-cross method, the oxidation
numbers are placed over the symbols for the elements just as before.
In this method, the oxidation numbers are then criss-crossed and used as the subscripts
for the other atom (ignoring sign).
This produces the correct formula
criss-cross error:
for the compound. Here’s an example of a
If you used the original method of finding the lowest multipliers to balance the charges,
you would get the correct formula
, but the criss-cross method produces the
incorrect formula
. If you use the criss-cross method to generate an ionic formula,
it is essential that you check to make sure that the subscripts correspond to the lowest
whole number ratio of the atoms involved. Note that this only applies to ionic
compounds. When we learn about covalent compounds in the chapter “Covalent Bonds
and Formulas,” you will see that the formula
describes a different molecule than
, so it would not be reduced to its simplest ratio.
Naming Ionic Compounds Practice Worksheet
Name the following ionic compounds:
1)
NH4Cl _____________________________________
2)
Fe(NO3)3 _____________________________________
3)
TiBr3 _____________________________________
4)
Cu3P _____________________________________
5)
SnSe2 _____________________________________
6)
GaAs _____________________________________
7)
Pb(SO4)2 _____________________________________
8)
Be(HCO3)2 _____________________________________
9)
Mn2(SO3)3 _____________________________________
10)
Al(CN)3 _____________________________________
Write the formulas for the following compounds:
11)
chromium (VI) phosphate ____________________________________
12)
vanadium (IV) carbonate ____________________________________
13)
tin (II) nitrite _____________________________________
14)
cobalt (III) oxide _____________________________________
15)
titanium (II) acetate _____________________________________
16)
vanadium (V) sulfide _____________________________________
17)
chromium (III) hydroxide _____________________________________
18)
lithium iodide_____________________________________
19)
lead (II) nitride _____________________________________
20
silver bromide _____________________________________
Lots of Ionic Naming Practice Problems
Name the following ionic compounds:
1)
NaBr __________________________________
2)
Sc(OH)3 __________________________________
3)
V2(SO4)3 __________________________________
4)
NH4F __________________________________
5)
CaCO3 __________________________________
6)
NiPO4 __________________________________
7)
Li2SO3 __________________________________
8)
Zn3P2 __________________________________
9)
Sr(C2H3O2)2 __________________________________
10)
Cu2O __________________________________
11)
Ag3PO4 __________________________________
12)
YClO3 __________________________________
13)
SnS2 __________________________________
14)
Ti(CN)4 __________________________________
15)
KMnO4 __________________________________
16)
Pb3N2 __________________________________
17)
CoCO3 __________________________________
18)
CdSO3 __________________________________
19)
Cu(NO2)2 __________________________________
20)
Fe(HCO3)2 __________________________________
Write the formulas for the following ionic compounds:
21)
lithium acetate __________________________________
22)
iron (II) phosphate __________________________________
23)
titanium (II) selenide __________________________________
24)
calcium bromide __________________________________
25)
gallium chloride __________________________________
26)
sodium hydride __________________________________
27)
beryllium hydroxide __________________________________
28)
zinc carbonate __________________________________
29)
manganese (VII) arsenide __________________________________
30)
copper (II) chlorate __________________________________
31)
cobalt (III) chromate __________________________________
32)
ammonium oxide __________________________________
33)
potassium hydroxide __________________________________
34)
lead (IV) sulfate __________________________________
35)
silver cyanide __________________________________
36)
vanadium (V) nitride __________________________________
37)
strontium acetate __________________________________
38)
molybdenum sulfate __________________________________
39)
platinum (II) sulfide __________________________________
40)
ammonium sulfate __________________________________
Mixed Ionic/Covalent Compound Naming
For each of the following questions, determine whether the compound is ionic or covalent and name it
appropriately.
1)
Na2CO3 _________________________________________
2)
P2O5 _________________________________________
3)
NH3 _________________________________________
4)
FeSO4 _________________________________________
5)
SiO2 _________________________________________
6)
GaCl3 _________________________________________
7)
CoBr2 _________________________________________
8)
B2H4 _________________________________________
9)
CO _________________________________________
10)
P4 _________________________________________
For each of the following questions, determine whether the compound is ionic or covalent and write the
appropriate formula for it.
11)
dinitrogen trioxide _________________________________________
12)
nitrogen _________________________________________
13)
methane _________________________________________
14)
lithium acetate _________________________________________
15)
phosphorus trifluoride _______________________________________
16)
vanadium (V) oxide _________________________________________
17)
aluminum hydroxide ________________________________________
18)
zinc sulfide _________________________________________
19)
silicon tetrafluoride _________________________________________
20)
silver phosphate _________________________________________
(Still) More Naming Practice
Write the names of the following chemical compounds:
1)
BBr3 ______________________________________
2)
CaSO4 ______________________________________
3)
C2Br6 ______________________________________
4)
Cr(CO3)3 ______________________________________
5)
Ag3P ______________________________________
6)
IO2 ______________________________________
7)
VO2 ______________________________________
8)
PbS ______________________________________
9)
CH4 ______________________________________
10)
N2O3 ______________________________________
Write the formulas of the following chemical compounds:
11)
tetraphosphorus triselenide ____________________________________
12)
potassium acetate ______________________________________
13)
iron (II) phosphide ______________________________________
14)
disilicon hexabromide ______________________________________
15)
titanium (IV) nitrate ______________________________________
16)
diselenium diiodide ______________________________________
17)
copper (I) phosphate ______________________________________
18)
gallium oxide ______________________________________
19)
tetrasulfur dinitride ______________________________________
20)
phosphorus ______________________________________
Review– Naming Chemical Compounds
The following are a good mix of naming and formula writing problems to help you get some practice.
Name the following chemical compounds:
1)
NaBr ______________________________________________
2)
Ca(C2H3O2)2 ______________________________________________
3)
P2O5 ______________________________________________
4)
Ti(SO4)2 ______________________________________________
5)
FePO4 ______________________________________________
6)
K3N ______________________________________________
7)
SO2 ______________________________________________
8)
CuOH ______________________________________________
9)
Zn(NO2)2 ______________________________________________
10)
V2S3 ______________________________________________
Write the formulas for the following chemical compounds:
11)
silicon dioxide ______________________________________________
12)
nickel (III) sulfide _____________________________________________
13)
manganese (II) phosphate _____________________________________
14)
silver acetate ______________________________________________
15)
diboron tetrabromide _________________________________________
16)
magnesium sulfate heptahydrate ________________________________
17)
potassium carbonate _________________________________________
18)
ammonium oxide ____________________________________________
19)
tin (IV) selenide ______________________________________________
20)
carbon tetrachloride __________________________________________
Solutions for the Naming
Ionic Compounds Practice
Worksheet
1)
2)
3)
4)
5)
6)
7)
8)
9)
10)
ammonium chloride
iron (III) nitrate
titanium (III) bromide
copper (I) phosphide
tin (IV) selenide
gallium arsenide
lead (IV) sulfate
beryllium bicarbonate
manganese (III) sulfite
aluminum cyanide
11)
12)
13)
14)
15)
16)
17)
18)
19)
20)
Cr(PO4)2
V(CO3)2
Sn(NO2)2
Co2O3
Ti(C2H3O2)2
V2S5
Cr(OH)3
LiI
Pb3N2
AgBr
Ionic Naming Practice
Problems - Solutions
1)
NaBr
sodium bromide
2)
Sc(OH)3
scandium hydroxide
3)
V2(SO4)3
vanadium (III) sulfate
4)
NH4F
ammonium fluoride
5)
CaCO3 calcium
carbonate
6)
NiPO4 nickel (III)
phosphate
7)
Li2SO3 lithium sulfite
8)
Zn3P2
zinc
phosphide
9)
Sr(C2H3O2)2
strontium acetate
10)
Cu2O
copper (I) oxide
11)
Ag3PO4
silver
phosphate
12)
YClO3 yttrium
chlorate
13)
SnS2
tin (IV)
sulfide
14)
Ti(CN)4 titanium (IV)
cyanide
15)
KMnO4 potassium
permanganate
16)
Pb3N2
lead
(II) nitride
17)
CoCO3 cobalt (II)
carbonate
18)
CdSO3 cadmium
sulfite
19)
Cu(NO2)2
copper (I) nitrite
20)
Fe(HCO3)2
iron
(II) bicarbonate
21)
lithium acetate
LiC2H3O2
22)
iron (II) phosphate
Fe3(PO4)2
23)
titanium (II) selenide
TiSe
24)
calcium bromide
CaBr2
25)
gallium chloride
GaCl3
26)
sodium hydride
NaH
27)
beryllium hydroxide
Be(OH)2
28)
zinc carbonate
ZnCO3
29)
manganese (VII)
arsenide
Mn3As7
30)
copper (II) chlorate
Cu(ClO3)2
31)
cobalt (III) chromate
Co2(CrO4)3
32)
ammonium oxide
(NH4)2O
33)
potassium hydroxide
KOH
34)
lead (IV) sulfate
Pb(SO4)2
35)
silver cyanide
AgCN
36)
vanadium (V) nitride
V3N5
37)
strontium acetate
Sr(C2H3O2)2
38)
molybdenum sulfate
Mo(SO4)3
39)
platinum (II) sulfide
PtS
40)
ammonium sulfate
(NH4)2SO4
Ionic/Covalent Compound
Naming Solutions
1)
Na2CO3
sodium carbonate
2)
P2O5 diphosphorus
pentoxide
3)
NH3
ammonia
4)
FeSO4
iron
(II) sulfate
5)
SiO2
silicon
dioxide
6)
GaCl3
gallium chloride
7)
CoBr2
cobalt
(II) bromide
8)
B2H4
diboron tetrahydride
9)
CO
carbon monoxide
10)
P4
phosphorus
11)
12)
13)
14)
15)
16)
17)
18)
19)
20)
dinitrogen trioxide
N2O3
nitrogen
N2
methane
CH4
lithium acetate
LiC2H3O2
phosphorus trifluoride
PF3
vanadium (V) oxide
V2O5
aluminum hydroxide
Al(OH)3
zinc sulfide
ZnS
silicon tetrafluoride
SiF4
silver phosphate
Ag3PO4
(Still) More Naming Practice Answers
1)
BBr3
boron
tribromide
2)
CaSO4
calcium sulfate
3)
C2Br6
dicarbon
hexabromide
4)
Cr(CO3)3 chromium
(VI) carbonate
5)
Ag3P
silver
phosphide
6)
IO2
iodine
dioxide
7)
VO2
vanadium (IV) oxide
8)
PbS
lead
(II) sulfide
9)
CH4
methane
10)
N2O3
dinitrogen trioxide
Write the formulas of the
following chemical compounds:
11)
tetraphosphorus
triselenide
P4Se3
12)
potassium acetate
KC2H3O2
13)
iron (II) phosphide
Fe3P2
14)
disilicon hexabromide
Si2Br6
15)
titanium (IV) nitrate
Ti(NO3)4
16)
diselenium diiodide
Se2I2
17)
copper (I) phosphate
Cu3PO4
18)
gallium oxide
Ga2O3
19)
tetrasulfur dinitride
S4N2
20)
phosphorus
P4
Answers – Naming Chemical
Compounds
1)
NaBr
sodium bromide
2)
acetate
Ca(C2H3O2)2
calcium
3)
P2O5
pentoxide
diphosphorus
4)
Ti(SO4)2
titanium(IV) sulfate
5)
FePO4
iron(III) phosphate
6)
K3N
potassium nitride
7)
SO2
dioxide
sulfur
8)
CuOH
copper(I) hydroxide
9)
Zn(NO2)2
zinc nitrite
10)
V2S3
vanadium(III) sulfide
Write the formulas for the
following chemical compounds:
11)
silicon dioxide
SiO2
12)
nickel (III) sulfide
Ni2S3
13)
manganese (II)
phosphate Mn3(PO4)2
14)
silver acetate
AgC2H3O2
15)
diboron tetrabromide
B2Br4
16)
magnesium sulfate
heptahydrate
MgSO4.7H2O
17)
potassium carbonate
K2CO3
18)
ammonium oxide
(NH4)2O
19)
tin (IV) selenide
SnSe2
20) carbon tetrachloride
CCl4
Chemical Bonding
Terms:
Physical and Chemical
Change Worksheet
True or False. If false, correct
the underlined portion of the
statement so that it is true.
1. A physical change is a
change of matter from one
form to another without a
change in chemical properties.
TRUE
2. A physical change is a
change that occurs when a
substance changes
composition by forming one
or more new substances.
FALSE-CHEMICAL
CHANGE
3. Color change is evidence
that a chemical change may
have occurred.
TRUE
4. Fizzing or foaming is
evidence that a chemical
change may have occurred.
TRUE
5. Production of light is
evidence that a physical
change may have occurred.
FALSE- CHEMICAL
CHANGE
6. Production of heat or light
is evidence that a chemical
change may have occurred.
TRUE
7. A change in odor is
evidence that a physical
change may have occurred.
FALSE- CHEMICAL
CHANGE
8. Chemical changes can be
reversed by physical changes.
FALSE- CHEMICAL
CHANGES CANNOT BE
REVERSED
Identify each of the
following as either a
Physical change (P) or a
chemical change (C).
1. You cut your hair. P
2. Making a peanut, pretzel
and cereal mixture. P
3. Baking soda reacts with
vinegar and forms a gas.
C
4. A piece of metal is bent in
half. P
5. An aspirin is crushed into
fine powder. P
6. Copper turns green when
exposed to the
environment. C
7. Two clear liquids are
mixed and a yellow color
forms. C
8. Baking cookies. C
9. Diamonds are used to
scratch glass. P
10. A tree burns to form
ashes. C
11. A piece of paper is
crumpled up. P
12. Water freezes to form ice.
P
13. Food spoiling. C
14. A candle burning. C
15. A candle melting. P
A Thought Experiment
A sealed flask of a clear,
colorless liquid is left sitting
on an interior sunny
windowsill. After about an
hour, there are droplets of a
clear liquid on the glass above
the solution, which has turned
yellow. After two hours, the
solution is dark brown with
clear, colorless droplets of
liquid on the glass. After
sitting on the windowsill for a
week, the walls of the flask
have a silvery lining and both
the solution and the droplets
are clear and colorless.
6. Which of the following is
not an indication that a
chemical reaction has
occurred?
(a) formation of liquid
droplets above the solution
(b) the solution color
changing from clear to yellow
(c) the solution color
changing from brown to clear
(d) formation of a silvery
metallic foil on the walls of
the flask
7. The formation of the
silvery lining is an
example of which of the
following indicators of
chemical change?
(a) evolution of a gas
(b) distinct color change
(c) precipitate formation
(d) temperature change
1. (Short answer) There is
only one reaction taking
place in the flask. What is
one possible reason for all
of the color changes?
The reaction is taking place
over time (in stages) as the
temperature changes due to
location and duration.
2. (Short answer) An
observant chemistry
student is enjoying a glass
of iced tea during lunch
(not in the lab!), and she
notices that the color of
her drink changes as the
ice in the glass melts. Is a
chemical reaction
occurring? Why or why
not?
No, a physical change is
occurring as the tea is
separating from the water.
This is happening as the ice
in the glass is melting.
Change of state is a physical
change.