Download TEST on Atomic Structure

PRACTICE – Final Exam
Name: ______________________
The Final Exam is six pages and has 60 questions - 109 points possible = 100 points + 9 Extra Credit
1) Complete the table below to convert between scientific notation and standard form 2 points
Standard Form
62.3 g (example)
Scientific Notation
6.23 x 101 g
1993 mL
0.0000072 kg
1.993 x 103 mL
7.2 x 10-6 kg
Standard Form
Scientific Notation
5.300 x 10-3 cm
2.68023 x 102 kg
6.71 x 10-4 L
0.005300 cm
268.023 kg
0.000671 L
2) Use <, >, or = for each of the questions below. 3 points
a) 9.8 m _<_ 9800 km
0.0098 km
9,800,000 m
b) 1 mL _>_ 0.010 cL
0.1 cL
0.1 mL
c) 3.5 g _=_ .0035 kg
0.0035 kg
3.5 g
3) Complete the table below – Note that the particles are not is the same order: 3 points
Charge
Location
AMU
0
In Nucleus
1
Neutron
1Electron Cloud
0
Electron
1+
In Nucleus
1
Proton
4) Draw the Lewis Structures for the following neutral atoms. 3 points
C
F
Si
He
Ga
Ba
6) Fill in the blanks using one of the following elements. Please note that each element may be used once, more
than once, or not at all. 10 points
K, Ca, Ga, C, As, O, Cl, Kr
__Ca___ is an example of metal
__ O __ is an example of a nonmetal
__ As ___ is an example of a metalloid
__ C ____ has 6 total electrons
__ O_ ___ has 6 valence electrons
__ K ____ has 1 valence electrons
__ Ca ___ is an Alkaline Earth Metal
__ Kr ___ is a Nobel Gas.
__ Cl __ is a Halogen
___ K __is an Alkali Metal
13) Look at each pair of elements below, select (circle) which element has the larger atomic radii:
Be or Ca
Na or P
N or B
2 points
14) Look at each pair of elements below, select (circle) which element has the higher ionization energy:
C or Si
F or Br
N or Li
2 points
15) Look at each pair of elements below, select (circle) which element has the higher electronegativity:
O or Se
P or Mg
N or F
2 points
9-10) Complete the following problems for Magnesium and Phosphorus 5 points
Magnesium (Neutral )
e-= 12
112__
Ve- =__2_
__
P+ =_12_
2 8 2
12
Ve- =_5__
__
e- _15_
P+ =_15_
2 8 5
12
.Mg .
Mg 2+
Magnesium
2+
e-= 10
__
Ve- =_8__
__
P+ = 12__
What must be done to make this
atom stable?
3
Phosphorus (Neutral)
New Ion
Symbol
Lewis
Structure
12
Lose two electrons
New Ion
Symbol
Lewis
Structure
.. P.. .
P 3-
3
3-
Phosphorus
Ve- =_8__
__
e-=18_
P+ =_15_
What must be done to make this
atom stable?
3
2 8
2 8 8
12
Gain three electrons
3
(A stable atom or ion must have a full valence shell = 8 valence e-)
Identify each as either ionic or covalent compounds and provide either the name or formula 5 points
You may find these prefixes
helpful for the questions below
mono-
di-
tri-
tetra-
penta
hexa-
hepta
octa-
nona-
deca-
1
2
3
4
5
6
7
8
9
10
Ionic or
Covalent
Covalent
(remember only covalent compounds have the prefixes above)
Ionic
Magnesium Fluoride
13) phosphorus trifluoride
Covalent
PF3
14) sulfur dioxide
Covalent
SO2
15) N2O5
Covalent
Dinitrogen Pentoxide
Ionic
Ca(NO3)2
Covalent
Carbon Monoxide
18) lead (IV) oxide
Ionic
PbO2
19) FeSO4
Ionic
Iron (II) Sulfate
11) dinitrogen trioxide
12) MgF2
16) calcium nitrate
17) CO
Name or Formula
N2O3
For the following questions, put your answer in the box ___ at the beginning of the question.
NOTE: There are no questions like these on the test, but make sure you understand this for other questions.
20)
_7a_ Which group of elements in the periodic table is known as the halogens?
21)
_4 _ Use the periodic table to determine the number of electrons in a neutral atom of beryllium.
22)
_35_ Use the periodic table to determine the number of protons in an atom of bromine.
23)
_13_ What is the mass number for a carbon atom that has 7 neutrons in its nucleus?
Moving from left-to-right across a period (row) of the periodic table,
24) TRUE or FALSE - the ionization energy of the elements generally decreases
25) TRUE or FALSE - the atomic radius of the elements generally decreases
NOTE: There are only 10 multiple choice questions on the test – MOST are SIMILAR to these questions below
_D__ 26) Which of the following is true about subatomic particles?
a. Electrons have no charge and have almost no mass.
b. Protons are negatively charged and the lightest subatomic particle.
c. Neutrons have a negative charge and are the lightest subatomic particle.
d. Electrons have almost no mass compared to the protons
_A__ 27) All atoms are ____.
a. neutral, with the number of protons equaling the number of electrons
b. neutral, with the number of protons equaling the number of electrons, which is equal to
the number of neutrons
c. positively charged, with the number of protons exceeding the number of electrons
d. negatively charged, with the number of electrons exceeding the number of protons
_B__ 28) The nucleus of all atoms ____.
a. always has the same number of neutrons and is considered neutral
b. are positively charged because of the positive charge of the protons
c. are negatively charged because of the negative charge of the neutrons
d. are positively charged and it occupies the vast majority of the volume of the atom.
_B__ 29) The sum of the protons and electrons in an atom equals the ____.
a. atomic number
b. charge of the atom
c. atomic mass
d. mass number
_A__ 30) Isotopes of the same element have different ____.
a. numbers of neutrons b. numbers of protons c. numbers of electrons
_B__ 31) All atoms of the same element have the same ____.
a. number of neutrons
b. number of protons
c. mass numbers
d. atomic numbers
d. mass
_D__ 32) Which of the following elements is in the same period as krypton?
a. helium
b. magnesium
c. nitrogen
d. bromine
_B__ 33) Of the elements Fr, Sb, Al, and Rn, which is a metalloid?
a. Fr
b. Sb
c. Al
d. Rn
_A__ 34) Which of the following statements is NOT true?
a. Atoms of the same element must always have the same mass
b. Atoms of isotopes of an element have different numbers of neutrons.
c. The nucleus of an atom has a positive charge.
d. Atoms are mostly empty space.
_B__ 35) Which of the following particles are free to drift in metals?
a. protons
b. electrons
c. neutrons
d. cations (the electrostatic force is between the e- and the cations)
_C__ 36) Which of the following pairs of elements is most likely to form an ionic compound?
a. chlorine and oxygen
c. aluminum and chlorine (ionic is metal and nonmetal)
b. nitrogen and sulfur
d. sodium and lithium
_A__ 37) What characteristic of metals makes them good electrical conductors? (electricity is a flow of charge)
a. They have mobile valence electrons.
c. They have mobile cations.
b. They have mobile protons.
d. Their crystal structures can be rearranged easily.
_C__ 38) Which of these elements does not exist as a diatomic molecule?
a. H
b. F
c. Ar
d. O (Argon is a noble gas and is stable- will not bond)
_C__ 39) How do atoms achieve noble-gas electron configurations in double covalent bonds?
a. Two atoms share one electron.
c. Two atoms share two pairs of electrons. (one bond = 2 e-)
b. Two atoms share two electrons.
d. One atom completely loses two electrons to the other atom.
_D__
40) When Group 6A elements form ions, they ____. (6A elements have six valence electrons)
a. lose two protons
b. gain two protons
c. lose two electrons
d. gain two electrons
_A__ 41) Which of the following is true about the composition of ionic compounds?
a. They are composed of anions and cations.
c. They are composed of cations only.
b. They are composed of anions only.
d. They are formed from two or more nonmetallic elements.
_A__ 42) Which element, when combined with bromine, would most likely form an ionic compound?
a. lithium
b. carbon
c. phosphorus
d. chlorine
(Ionic = metal (lithium) and a nonmetal (bromine))
_A__ 43) Which of the following occurs in an ionic bond? (electrostatic forces between charged ions)
a. Oppositely charged ions attract.
c. Two atoms share more than two electrons.
b. Two atoms share two electrons.
d. Like-charged ions attract.
_A__ 44) Which of the following pairs of elements is most likely to form an ionic compound?
a. magnesium and fluorine
c. oxygen and chlorine
(ionic = metal and nonmetal)
b. nitrogen and sulfur
d. sodium and aluminum
_A__ 45) A bond formed between a calcium atom and an oxygen atom is likely to be ____.
a. ionic
b. coordinate covalent
c. polar covalent
d. nonpolar covalent
(Ionic = metal (calcium) and nonmetal (oxygen))
_A__ 46) Which of the following covalent bonds is the most polar? (more polar = larger difference in EN)
a. H—F
b. H—C
c. H—H
d. H—N (Fluorine has the highest Electronegativity (EN))
_C__ 47) Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen?
a. C
b. Na
c. O
d. S (Oxygen has the highest electronegativity (EN))
_B__ 48) Which of the forces of molecular attraction is the weakest? (dispersion is just from the moving e-)
a. dipole interaction
b. dispersion
c. hydrogen bond
d. single covalent bond
49) Compare and Contrast Ionic and covalent bonds. 3 points
Both allow for stable atoms or ions. They both involve electrons. They are
both electrostatic forces between opposite charges. Both may involve nonmetals.
a) how are they similar?
b) how are they different?
Ionic
~ transferring electrons
~ metal & nonmetal
~ attraction between ions
Covalent
~ sharing electrons
~ two nonmetals
~ attraction between neutral atoms
and the electrons between them.
105) Complete the Lewis Structures for each Compound (there will be two of these) 4 points
Cl2 ____________
C2H4 ___________
N2 ____________
Cl – Cl (single bond)
N
N (triple bond)
(NOTE: I will provide you with a copy of the electronegativities of the atoms)
Identify each of the Bond Types as either: Nonpolar Covalent, Polar Covalent, or Ionic
(Do not forget to include the identification of cations and anions or partial positive and partial negative where appropriate.)
(for ionic)
(for polar covalent)
4 points
51) HO
H
2.2
O
3.5
ΔEN =
52) NaI
1.3
Na
0.9
Polar Covalent
53) HC
H
2.2
C
2.5
F
4.0
O
3.5
I
2.5
-
ΔEN =
1.6
Ionic
ΔEN =
54) H-H
0.3
H
2.2
H
2.2
ΔEN =
0.0
Nonpolar Covalent
Nonpolar Covalent
55) FO
+
ΔEN =
0.5
Polar Covalent
56) HN
H
2.2
N
3.0
ΔEN =
0.8
Polar Covalent
Identify each of the following as either intermolecular or intramolecular
2 points
57) _ intramolecular__ Polar Covalent Bond
60) _ intramolecular__ Ionic Bond
58) _ intermolecular__ Hydrogen Bond
61) _ intermolecular__ Dipole-Dipole Interact
59) _ intermolecular__ London Dispersion
62) _ intermolecular__ Van der Waals
Intramolecular = between Atoms intermolecular = between molecules
63) Explain “why” atoms become partially positive and partially negative in a polar bond.
2 points
In a polar bond, the difference between the electronegativities between the two non-metals is
greater than 0.4, this difference will result in the shared electrons not being shared equally.
This unequal sharing will cause the electrons to move closer to the atom with the higher
electronegativity. The negatively charged electrons will result in this higher electronegative
atom becoming partial negative, and the other atom becoming partial positive.
1 m3 = 1,000 L
1 mL = 1 cm3
1 inch = 2.54 cm
1 mile = 5280 ft
1 Atm = 101.3 kPa = 760 mmHg = 14.7 PSI
1 km = 1,000 m
1 m = 100 cm = 1,000 mm
1 kg = 1,000 g
1 g = 100 cg = 1,000 mg
1 kL = 1,000 L
1 L = 100 cL = 1,000 mL
1 lb = 454 grams
1oz = 28.35 g
1 lb = 16 oz
1 quart = 0.95 L
1 gallon = 4 quarts
1 quart = 2 pints
1 pint = 2 cups
1 cup = 8 oz. (fl)
Perform the following conversions: (Show your work to earn partial credit) Missing units = loss of credit
NOTE: There will be five problems like those below (64-71)
64) 147.2 kPa = ____ mmHg
x
760 mmHg
101.3 kPa
65) 3.4 Atm = ____ kPa
x
101.3 kPa
1 Atm
66) 894.2 cm = ____ km
x
1m .
100 cm
67) 287,520 mg = ____ kg
x
1g .
1000 mg
68) 97 mL to gallons
x
1L .
1,000 mL
69) 133.5 mm to inches x
100 cm .
1,000 mm
= 344 kPa
x
x
x
= 1104 mmHg
x
1 km .
1,000 m
= 0.008942 km
1 kg .
1,000 g
1 qt .
0.95 L
x
= 0.28752 kg
1 gal
4 qt
1 in .
2.54 cm
= 0.0255 gallons
= 5.256 inches
NOTE: You will need to know Avagadro’s Number for the following two questions
70) How many atoms of platinum are in the 4.2 g ring? (From Periodic Table: 1 mole Pt = 195.08 g Pt)
4.2 g
x
1 mole .
195.08 g
x
6.022 x 1023 atoms
1 mole
= 1.3 x 1022 atoms of platinum
71) If there are 5.45 x 1025 atoms of aluminum (Al), how many grams would this be? (1 mole = 26.98g)
5.45 x 1025 atoms
x
1 mole
.
6.022 x 1023 atoms
x
26.98 g .
1 mole
= 2442 grams of aluminum
4points
72) TRUE or FALSE: The motion/speed of the particles increases as the temperature of particles decreases.
73) TRUE or FALSE: Because the shape of a solid never changes, the particles of the solid do not move.
74) TRUE or FALSE: Particles can stick together because of the intermolecular forces between the particles.
75-78) Balance the following equations 2 points
[3] C + [ 4] H2  [ 1] C3H8
[4] NaI + [1] Pb(SO4)2
[2] Fe(OH)3  [1] Fe2O3 + [3] H2O

[1] PbI4 + [2] Na2SO4
[1] H3PO4 + [3] NaBr  [3] HBr + [1] Na3PO4
3 points
79) Look at the equations in questions 75-78 above. List each chemical as either a reactant (R) or a product (P).
C
PbI4
Fe(OH)3
NaBr
NaI
H2O
C3H8
H2
R
Prod
R
R
R
Prod
Prod
R
80) How does the Law of Conservation of Mass relate to balancing chemical equations? 2 points
The law of conservation of mass states that matter can not be created or destroyed. By balancing a
chemical equation the number and type of atoms in the REACTANTS are the EXACT same number and
type of atoms in the PRODUCTS.
81-85) Write balanced equations for the following word equations. Indicate the type of reaction on the line to
the left of the equation by classifying each reaction as single replacement (SR), double replacement (DR),
decomposition (D), synthesis (S), or combustion (C). (NO PHASE LABELS) 4 * 3 points each = 12 points
_S_81) phosphorous + oxygen 
diphosphorous trioxide
P
+
O2

P2O3 (No ions as it is a covalent compound)
4 P
+
3 O2 
2 P2O3
.
1 point for the type of reaction, 1 point for writing compounds with a net charge of zero, and 1 point for balancing
_ DR 82) lithium nitride + barium nitrate 
lithium nitrate + barium nitride
1+
32+
1Li N
+
Ba NO3

Li1+ NO31+ Ba2+ N32 Li 3N
+
3 Ba(NO3 )2 
6 LiNO3
+ 1 Ba3N2
_ DR 83) sodium bromide +
Na1+ Br1+
2 NaBr
+
.
(make sure you write the names of the products)
calcium hydroxide  sodium hydroxide + calcium bromide
.
Ca2+ OH1
Na1+ OH1+
Ca2+ Br11 Ca(OH)2

2 NaOH
+
1 CaBr2
_DR 84) Solutions of potassium chloride and silver nitrate are mixed to create solid silver chloride and
aqueous potassium nitrate.
K1+ Cl 1- + Ag1+ NO31- 
Ag1+ Cl 1- +
K1+ NO31_1_ KCl (aq) + _1_ Ag NO3(aq)  _1_ AgCl (s) + _1_ KNO3 (aq)
_DR 85) Aqueous ammonium hydroxide reacts with aqueous copper (II) nitrate to produce solid copper (II)
hydroxide and a solution of ammonium nitrate.
NH41+ OH1- +
CU2+ NO31
CU2+ OH1- +
NH41+ NO31_2_ NH4OH (aq) + _1_ CU(NO3)2 (aq)  _1_ CU(OH)2 (s) + _2_ NH4NO3 (aq)
86) List the seven diatomic elements. 2 points
H2
N2
O2
F2 Cl2
Br2
I2
87) How did you know that a chemical reaction occurred when you added the magnesium metal to the
solution of hydrochloric acid? 2 points
Bubbling occurred, this bubbling was a release of a gas . The production of a gas is one source of
evidence that a chemical reaction is occurring.
88) How many grams of lead (II) phosphate will be formed when 85.39 grams of phosphoric acid (H3PO4)
react with an excess of lead metal in the following reaction? 5 points
_3__ Pb + _2__ H3PO4  _3__ H2 + _1__ Pb3(PO4)2
MM = Pb3(PO4)2 = 3(207.2 g) + 2(30.97 g) + 8(16.00 g) = 811.54 g/mol Pb3(PO4)2
MM = H3PO4= 3(1.01 g) + 1(30.97 g) + 4(16.00 g) = 98.00 g/mol H3PO4
1 mol H3PO4
85.39 g H3PO4
1 mol Pb3(PO4)2
811.54 g Pb3(PO4)2
x ------------------ x ----------------- x -----------------98.00 g H3PO4
2 mol H3PO4
=
353.56 g
Pb3(PO4)2
1 mol Pb3(PO4)2
5 points = 1 point for balancing, 2 points for molar masses, and 2 points for final mass (stoichiometry)
89) How many grams of hydrofluoric acid (HF) are required to react completely with 23.68 grams of calcium
hydroxide in the following reaction? 5 points
_1_ Ca(OH)2 + __2_ HF  __1_ CaF2 + __2_H2O
MM = HF = 1(1.01 g) + 1(19.00 g) = 20.01 g/mol HF
MM = Ca(OH)2 = 1(40.08 g) + 2(16.00 g) + 2 (1.01 g) = 74.10 g/mol Ca(OH)2
1 mol Ca(OH)2
23.68 Ca(OH)2
2 mol HF
20.01 g HF
x ------------------ x ----------------- x ------------------ = 12.79 g HF
74.10 g Ca(OH)2
1 mol Ca(OH)2
1 mol HF
NOTE: There are eleven more points/questions that are based on reaction rates
Final Exam is six pages and has 60 question: 109 points possible = 100 points + 9 Extra Credit
You are allowed to use TWO index cards (BOTH SIDES) or ONE SIDE of a piece of paper:
a) TWO index cards (front and back) OR
b) ONE piece of standard sized typing paper (only ONE SIDE of the paper)
Similar to all of my tests and quizzes, the questions on your FINAL EXAM will be similar to these provided on
this practice test. I recommend that you look over your old tests, old practice tests, old quizzes, old notes, old
homework assignments… to help you prepare for the final exam. I am almost always available for questions.