WorksheetsFall Semester Review II
Total questions: 66
Worksheet time: 1hrs 17mins
Name
Class
Date
1.
What is the correct electron configuration for Boron
a)
1s22s22p1
b)
1s22s22p2
c)
1s22s11p1
d)
1s22s12p1
2.
Which element is depicted from this atomic orbital diagram?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Phosphorus
3.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
4.
What atom matches this electron configuration?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
5.
1. What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
6.
What is the shape of a p orbital?
a)
sphere
b)
it's just too complex to thing about it
c)
dumbbell
d)
I don't know this stuff.
7.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
8.
What atom is represented here?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Fluorine
9.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
10.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
11.
What is the electron configuration for this atom?
a)
1s22s22p6
b)
1s22s22p5
c)
1s22s22p3
d)
2s22p3
12.
What is incorrect about the Lewis structure?
a)
too many valence e-
b)
too few valence e-
c)
paired e- with not all sides filled
d)
nothing
13.
How many electrons should Potassium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
14.
What is the noble gas shorthand for Sulfur?
a)
[Ar]3p4
b)
[He]3s23p4
c)
[Ne]3s23p4
d)
[Na]3s23p4
15.
Which is a correct orbital box diagram?
a)
a
b)
b
c)
d
d)
e
16.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
17.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
18.
Which of the following shapes has unshared pairs of electrons on the central atom?
a)
Trigonal Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
19.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
20.
Which shapes are altered by unshared pairs of electrons?
a)
Bent and Trigonal Pyramidal
b)
Trigonal Planar and Bent
c)
Tetrahedral andTrigonal Bipyramidal
d)
Trigonal Pyramidal and Linear
21.
How many unshared pairs of electrons will a bent molecule, such as water, have?
a)
1
b)
2
c)
3
d)
4
22.
How many unshared pairs of electrons will a trigonal pyramidal molecule have?
a)
1
b)
2
c)
3
d)
4
23.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
24.
Who could this be?
a)
CO2
b)
NH3
c)
H2S
d)
CH4
25.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
26.
What shape would PH3 have?
a)
Trigonal Planar
b)
Trigonal Pyramidal
c)
Bent
d)
Trigonal Bipyramidal
27.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
28.
Defining ionic compounds: Which of the following groups contains no ionic compounds?
a)
HCN, NO2, Ca(NO3)2
b)
KOH, CaF2, NaNH2
c)
PCl5, LiBr, Zn(OH)2
d)
CH2O, H2S, NH3
29.
Ionic vs. Covalent Rules: What is the formula for magnesium nitrate
a)
Mg(NO3)2
b)
MgNO3
c)
Mg2(NO3)2
d)
Mg2(NO3)
30.
Ionic vs. Covalent Rules: What is the formula for carbon hexasulfide?
a)
CS6
b)
C6S6
c)
CS
d)
CS2
31.
Ionic vs. Covalent Rules: What is the name for the compound K2SO4
a)
potassium sulfate
b)
potassium disulfide
c)
dipotassium sulfate
d)
potassium sulfur oxide
32.
Determining charges: What is the name for FeN?
a)
Iron (III) nitride
b)
Iron (II) nitride
c)
Iron nitrate
d)
Iron (III) nitrate
33.
Determining charges: Cr3N
a)
chromium nitride
b)
chromium (I) nitride
c)
chromium (II) nitride
d)
chromium (III) nitride
34.
Drawing Lewis Structures: What kind of bond does a diatomic nitrogen molecule have?
a)
single covalent
b)
double covalent
c)
triple covalent
d)
ionic
35.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
36.
How many neutrons does the isotope of lithium-8 have?
a)
8
b)
3
c)
4
d)
5
37.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
38.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
39.
Negative ions form when atoms _________ valence electrons.
a)
lose
b)
gain
c)
share
40.
Group 17 always has ions with a charge of
a)
+1
b)
+2
c)
-1
d)
-2
41.
True or false: as you move along the spectrum, left to right, the wavelengths decrease in size (get smaller)
a)
true
b)
false
42.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
43.
Select the correct order of waves on the EMS
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
44.
Which has the LONGEST wavelength and, therefore, the lowest frequency/energy
a)
Gamma Rays
b)
Radio Waves
c)
Visible Light
d)
Infrared rays
45.
Which has the SHORTEST wavelength and, therefore, the highest frequency/most energy
a)
Radio waves
b)
Ultraviolet Rays
c)
Gamma Rays
d)
X-rays
46.
Put the visible light colors in order from longest wavelength to shortest wavelength
a)
Violet, Indigo, Blue, Green, Orange, Yellow, Red
b)
Red, Yellow, Green, Orange, Violet, Blue, Indigo
c)
Red, Orange, Yellow, Green, Blue, Indigo, Violet
47.
Light is emitted when an electron moves from the ________ state to the _________ state
a)
excited, ground
b)
ground, excited
48.
Which color has the least amount of energy?
a)
red
b)
orange
c)
green
d)
blue
49.
Which color has the highest frequency?
a)
red
b)
orange
c)
green
d)
blue
50.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
51.
The mass of one mole of substance is called...
a)
molecular mass
b)
mole constant
c)
molar mass
d)
atomic weight
52.
What is the mass of one mole of aluminum chloride (remember to determine the correct formula first)?
a)
62.435g
b)
116.399g
c)
133.341g
d)
97.888g
53.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
54.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
55.
The mass of one mole of substance is called...
a)
molecular mass
b)
mole constant
c)
molar mass
d)
atomic weight
56.
What are the units for molar mass?
a)
grams
b)
moles
c)
grams/mole
d)
liters
57.
Fluorine gas is diatomic. What is its molar mass?
a)
18.998 g/mol
b)
37.996 g/mol
c)
9 g/mol
d)
18 g/mol
58.
What is the molar mass of B2(CO3)3?
a)
81.632 g/mol
b)
94.842 g/mol
c)
38.822 g/mol
d)
201.648 g/mol
59.
What is the percent composition of a compound that contains 40.8 g carbon and 54.4 g oxygen?
a)
42.9 % carbon; 57.1% oxygen
b)
57.1 % carbon; 42.9 % oxygen
c)
40.8 % carbon; 54.4 % oxygen
d)
54.4 % carbon; 40.8% oxygen
60.
The minimum energy required to remove an electron from the ground state of an atom
a)
electron configuration
b)
energy levels
c)
ionization energy
d)
ionic bond
61.
Which has the greater EN:
Cl or Al?
Cl or Al?
a)
Cl
b)
Al
62.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
63.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
64.
Which is larger:
Ca or Ca+2
Ca or Ca+2
a)
Ca
b)
Ca+2
c)
both are same size
65.
Which is larger:
P or P-3
P or P-3
a)
P
b)
P-3
c)
both are same size
66.
The element with the lowest electronegativity in Period 3 is -
a)
Na
b)
Cl
c)
Ar
d)
Mg
100 %
