Review Practice Problems Part #1: Topics 1-6
2
Who were the 10 scientists that were
covered in class that contributed to the
development
of different
Sketch
and name
the fouratomic
atomic models
models?
did in
they
each
that wereWhat
covered
class.
contribute?
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Describe Rutherford’s Gold Foil
experiment and what it proved.
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4
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7
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10
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Bohr
Rutherford observed how an alpha particle beam was scattered when it stroke a thin gold foil. It
proved the existence of a small massive center to atoms, which would later be known as the nucleus
of an atom.
What does the Quantum model say about Orbital quantum numbers tell you what energy level the electron is in, and the types of orbital tell
the nature of electrons in an atom?
you shapes of orbitals (sometimes called electron clouds), volumes of space in which there is likely
to be an electron.
Put 0.00345 in scientific notation
3.45×10-3
Put 29800000 in scientific notation
2.98×107
What is wrong with the following
number that was supposed to be put in
sci. notation? 24.6 x 103
What is wrong with the following
number that was supposed to be put in
sci. notation? 0.54 x 102
What is the definition of atomic mass?
24.6 is greater than 10.
It should be 2.46×104
How many neutrons does an atom of
silver-108 have?
How many protons, neutrons, and
electrons does each atom have? Cl-35
Ba-137 C-12 Ne-20
When mass number is 108, there are 61 neutrons because the proton number is 47.
108-47=61
Cl
Ba
C
Ne
p
17
56
6
10
n
18
81
6
10
e
17
56
6
10
each of two or more atoms of the same element that contain equal numbers of protons but different
numbers of neutrons in their nuclei.
Carbon-12 has 6 neutrons, Carbon-13 has 7 neutrons, and Carbon-14 has 8 neutrons
14
What is the difference between Carbon12, Carbon-13, and Carbon-14?
How many protons, neutrons,
electrons does Bromine-80 have
compared to Bromine-83?
Which version of Bromine above is the
more common isotope? How do you
know?
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What is a mole?
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Why do we use “the mole” in chemistry
class?
What’s the difference between
observation and interpretation?
Qualitative observation vs
quantitative observation?
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the mass of an atom of an element expressed in atomic mass units (amu)
Number of protons of the atom
What is an isotope?
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0.54 is lower than 1
It should be 5.4×101
What does the atomic number tell you?
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Aristotle, Democritus, John Dalton, J. J. Thomson, Rutherford, Neils Bohr, de Broglie,
Heisenberg, SchrÖdinger, Chadwick
Dalton
Bromine-80 has 35 protons, 45 neutrons, and 35 electrons
Bromine-83 has 35 protons, 48 neutrons, and 35 electrons
Bromine-80 is the more common isotope because the average atomic mass for Bromine is 79.90
amu, which is closer to 80 amu.
A mole is the quantity of anything that has the same number of particles, which is which is roughly
6.02×1023
Moles give us a consistent method to convert between atoms/molecules (too small and too many to
be counted) and grams (easily be measured).
An observation is any report from your 5 senses. It does not involve an explanation. An
observation can also involve measurements. Such an observation is a quantitative one, as
opposed to a qualitative one (no measurements). On the other hand, an interpretation is an
attempt to figure out what has been observed.
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What is density? How do you calculate
it? What is its unit?
The density of a substance is the relationship between the mass of the substance and how much
space it takes up (volume). Density equals the mass of the substance divided by its volume: D = m/v.
The unit is g/cm3 or g/mL
21
How do you read a phase diagram and
what a phase diagram can tell you?
The phase diagram shows, in pressure–temperature, the lines of equilibrium or phase boundaries
between the three phases of solid, liquid, and gas. Single phase regions are separated by lines where
phase transitions occur, which are called phase boundaries. Triple point is the temperature and
pressure at which the three phases (gas, liquid, and solid) of that substance coexist.
22
What are the differences between
chemical and physical changes?
A physical change in a substance doesn't change what the substance is. In a chemical change where
there is a chemical reaction, a new substance is formed and energy is either given off or absorbed.
Physical changes can be reversed, but chemical changes cannot.
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What are the signs of a chemical
reaction?
Change in color, change in temperature, formation of gas bubbles, and formation of a solid
(precipitate)
Review Practice Problems Part #2: Topics 7-12
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7
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10
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14
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What is an electron orbital?
Sketch pictures of an “s” orbital and a
“p” orbital.
How many electrons can an orbital
hold?
How many electrons can a set of s
orbitals hold? A set of p orbitals? A
set of d orbitals? A set of f orbitals?
Sketch what the orbital diagram
should look like for sulfur.
Write a short paragraph explaining
how to fill an orbital diagram.
What element is represented by the econfiguration of:
1s22s22p63s23p64s23d104p2 ?
What element is represented by the
electron configuration of:
1s22s22p63s23p64s1
Write the electron configuration for
phosphorus
s-2, p-6, d-10, f-14
S
Mg
fill the lowest energy level first, maximum of 2 electrons with opposite spin may be
placed in each orbital, and 1 electron is added to each sub energy level before double up
Germanium (Ge)
Potassium (K)
1s22s22p63s23p3
Write the electron configuration for
1s22s22p63s23p64s23d104p65s14d10
silver
Draw a picture of what happens during
atomic absorption. Write 3 sentences
describing what happens.
Electrons in an atom absorb energy, get excited
and jump from a ground state up to higher energy
levels (excited state).
Energy is released when electrons in an atom
Draw a picture of what happens
come back down from an excited state of higher
during atomic emission. Write 3
energy level to a ground state of lower energy
sentences describing what happens.
level
What does ground state mean? Excited A ground state atom possesses electrons in its lowest energy orbitals. Excited state means
state?
a valence electron absorbs energy and jumps up to a higher energy level.
List the three main types of radiation, Alpha, α, 42α, 42He, a piece of paper
what their symbols are (including the Beta, β, 0-1β, 0-1e, a piece of thin metal
little numbers on top and bottom of
Gamma, γ, 00γ, a thick layer of heavy metal like lead.
the symbol), and what stops them.
18
19
Finish the following nuclear equation:
238
234
U 
Th +
20
Write the nuclear equation for
Samarium undergoing beta emission
17
2
Sketch what the orbital diagram
should look like for Mg
Which type of radiation is pure
energy? Which type is a high energy
electron? Which type is a helium
nucleus?
What is the charge on the three main
types of radiation & what type of
charge would they be attracted to?
Finish the following nuclear equation:
99
+ 0-1e
43Tc → _
16
Electronic orbitals are regions within the atom in which electrons have the highest
probability of being found.
Gamma is pure energy, beta is a high energy electron and alpha is a helium nucleus.
Alpha, +2, attracted to negative charge
Beta, -1, attracted to positive charge
Gamma, 0, attracted to neither.
99
99
+ +0 10e-1e
43Tc → 44Ru
4
3
238
234
4
92U →
90Th + 2α
9
2
9
0
146
146
0
62Sm →
63Eu + -1β
Review Practice Problems Part #3: Topics 13-19
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What charge do alkali metals, alkaline earth metals,
halogens, oxygen group like to have? (example,
alkalimany
metalsvalence
like to electrons
have +1 charge)
How
does each of the
following have: Na, Cs, Be, F, O, S, C, B
Alkali: +1;
Alkaline earth metals: +2;
Halogens: -1;
Oxygen group: -2
Na (1), Cs (1), Be (2), F (7), O (6), S (6), C (4), B (3)
Write the symbol for a particle with 17 protons, 18
neutrons, and 18 electrons
List two of each type of atom: metals, nonmetals,
metalloid, and transition metals
Draw a sketch of a periodic table and draw an
arrow pointing from lowest ionization energy
towards the highest.
35
Rank the atoms from lowest to highest ionization
energy: Na, F, Fr, Ca, Fe, S
Draw a sketch of a periodic table and draw an
arrow pointing from lowest electronegativity
towards the highest.
Fr, Na, Ca, Fe, S, F
Rank the following atoms from lowest to highest
electronegativity: Na, F, Fr, Ca, Fe, S
Draw a sketch of a periodic table and draw an arrow
pointing from smallest to largest atomic radius.
Fr, Na, Ca, Fe, S, F
Rank the following atoms from smallest to largest
atomic radius: Na, F, Fr, Ca, Fe, S
Describe how to name ionic compounds vs covalent
molecules
Name the following: N4O10 P4S10 MgCl2 CCl4
C5I Al2O3 SrSO4 NH4Cl Ca(NO3)2
F, S, Fe, Na, Ca, Fr
Write the formula for the following: Gallium Oxide,
Calcium Chloride, Ammonium Chloride, Calcium
Fluoride
Write the formula for diphosphorus monoxide,
tetrasulfur trifluoride, nitrogen tetrahydride
What types of elements make up ionic bonds?
Covalent bonds? How do you decide a covalent bond
as polar or nonpolar?
What is happening during an ionic bond? A covalent
bond? Why do things bond in the first place???
17
Identify the following as ionic, or covalent:
NaF
KOH CS2 NO
H2
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What is the definition of the octet rule?
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What are the main exceptions to the octet rule?
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23
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F2
Draw Lewis Structures for CO2, N2, O2, H2, H2O,
NH3
For the Lewis Structures you drew above identify
which have single bonds, double bonds, triple bonds.
Calculate the average atomic mass of sulfur if
95.00% of all sulfur atoms have a mass of 31.972
amu, 0.76% has a mass of 32.971amu and 4.22%
have a mass of 33.967amu.
How to calculate %yield and %error in the copper
cycle lab?
What are the 5 types of chemical reactions? Write a
generic equation for each type of reactions.
Explain the role of bond breaking and bond forming
in a chemical reaction and overall absorption or
production of heat energy (endothermic or
exothermic reaction).
17Cl
-
List any two of each. The following are just examples.
Metals: Na, Ca; Nonmetals: O, Cl; Metalloid: Si, Ge;
Zn
Transition metals: Cu,
Ionic compounds: name cation first, then anion (finish with –ide). DO NOT use prefix
Covalent molecules: use prefix except when the first element is one.
N4O10-tetranitrogen pentoxide; P4S10-tetraphosphorus decasulfide; MgCl2-magnesium
chloride; CCl4-carbon tetrachloride; C5I-pentacarbon monoiodide; Al2O3-aluminum oxide;
SrSO4-strongtium sulfate; NH4Cl-ammonium chloride; Ca(NO3)2-calcium nitrate
Gallium Oxide: Ga2O3, Calcium Chloride: CaCl2, Ammonium Chloride: NH4Cl,
Calcium Fluoride: CaF2
diphosphorus monoxide: P2O , tetrasulfur trifluoride: S4F3, nitrogen tetrahydride: NH4
Metal & nonmetal make up ionic bonds. Nonmetal & nonmetal make covalent bonds.
When electronegativity difference of the 2 nonmetals is very small (<0.4), the covalent
bond is nonpolar; If the difference is between 0.4-1.6(roughly) it’s polar.
Electrons are transferred from metal to nonmetal in an ionic bond; electrons are
shared between 2 nonmetals in a covalent bond. Things bond because they have an
attraction force between them.
Ionic: NaF KOH
Covalent: CS2
NO H2 F2
When atoms combine to form compounds they generally each lose, gain, or share valence
electrons to attain an electron configuration of the nearest noble gas (8 valence electrons).
Hydrogen only needs 2 valence electrons to be stable.
H-H
CO2 has 2 double bonds, N2 has 1 triple bond, O2 has 1 double bond, H2 has 1single
bond, H2O has 2 single bonds, NH3 has 3 single bonds.
Average mass = (31.972×0.95) + (32.971×0.0076) + (33.967×0.0422) = 32.06 amu
%yield = recovered Cu mass/initial Cu mass × 100
%error = (initial Cu mass-recovered Cu mass)/initial Cu mass ×100 = 100-%yield
Synthesis A+B→AB; Decomposition ABC→AB + C;
Single replacement A+BX→AX+B; Double replacement AX+BY→AY+BX;
Combustion CxHy+O2→CO2+H2O
energy is absorbed to break bonds in reactants, and released when new bonds are formed
in products. If overall total energy is positive, meaning energy absorbed is higher than
energy released, it’s an endothermic reaction. If overall total energy is negative,
meaning energy released is higher than energy absorbed, it’s an exothermic reaction.