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Semester review part 2

Total questions: 84

Worksheet time: 3hrs 25mins

Name
Class
Date
1.
The Olympic record for the high jump is just over 2.6 yards. What is that distance in feet?  (3 ft=1 yd)
a)
0.867 ft
b)
7.8 ft
c)
8.07 ft
d)
8.27 ft
2.

Which conversion factor would be needed?

a)
b)
c)
d)
3.
You know 1000 mg = 1 g.  Convert 2.5 grams into milligrams.
a)
25 mg
b)
25,000 mg
c)
250 mg
d)
2500 mg
4.

Americans drink 5,604,000 gallons of sweet tea each day. How many liters is that? (1 gal = 3.79 L)

a)

21,200,000 L

b)

21,240,000 L

c)

21,207,190.2 L

d)

21,000,000 L

5.
What conversion factor would you use to solve this problem?
a)
2.20 lbs / 1 kg
b)
1 kg / 2.20 lbs
c)
0.002 lbs / 1 g
d)
1 g / 0.002 lbs
6.

Santa Maria has an elevation of 6.30 X 105 mm. How many Mm is this elevation?

a)

6.30 X 102 Mm

b)

6.3 X 10-2 Mm

c)

0.00063 Mm

d)

0.000630 Mm

7.

This past summer our rain gauge collected 0.80 yards of rain. Express this amount in centimeters.

a)

73 cm

b)

73.2 cm

c)

74 cm

d)

73.152 cm

8.

How many grams are equivalent to 1.800 X 10-4 tons?

a)

163.30 g

b)

163.296 g

c)

164 g

d)

163.3 g

9.

This is a broad range of radiation that carries energy in the form of waves

a)

Wavelength

b)

Frequency

c)

Energy

d)

Electromagnetic Spectrum

10.

When two different variables do the opposite thing

a)

Direct relationship

b)

Inverse relationship

11.

When two variables do the same thing (increase or decrease together)

a)

Direct relationship

b)

Inverse relationship

12.

  1. Which two variables of the electromagnetic spectrum have a direct relationship?
    (there may be more than one correct answer)

a)

Crests and trough

b)

Energy and frequency

c)

Wavelength and energy

d)

Frequency and wavelength

13.

  1. As wavelength increases, frequency __________ and energy ________.

a)

Increases, decreases

b)

Increases, increases

c)

Decreases, decreases

d)

Decreases, increases

14.

Which of the following best explains why ultraviolet rays can cause sunburn but visible light from a light bulb does not damage skin?

a)

Ultraviolet rays come before the visible light in the EM spectrum, which means anything before visible light automatically causes cancer.

b)

Ultraviolet rays have lower frequencies than visible light rays and thus have higher energy than light rays from a light bulb.

c)

Ultraviolet rays have higher frequency than visible light rays and thus have more energy than light rays from a light bulb.

d)

Ultraviolet rays have higher frequencies than visible light rays and thus have less energy than light rays from a light bulb.

15.

  1. The visible light that we can see travels in waves. Blue light has a wavelength of 450 nm and orange light has a wavelength of 600 nm. Based on this information, what is true about the energies of blue and orange light? 

a)

  1. Energy of blue light will be lower than that of orange light.

b)

  2. Energy of blue light will be higher than that of orange light.

c)

  2. Energy of blue light and orange light will be the same.

d)

  1. Wavelengths of light and energy of light are independent of each other.

16.

Which has a longer wavelength?

a)

Red

b)

Orange

c)

Blue

d)

Violet

17.

Which of these elements has the greatest atomic radius?

a)

H

b)

N

c)

Cl

d)

Cs

18.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
19.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
20.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
21.

Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?

a)

beryllium, Be

b)

potassium, K

c)

titanium, Ti

d)

yttrium, Y

22.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
23.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
24.

The common charge on an atom in group 17 would be....

a)

+1

b)

+7

c)

-7

d)

-1

e)

17

25.

What BEST DESCRIBES a spontaneous or natural liking?

a)

Affinity

b)

Ionization

c)

Discharge

d)

Polarity

26.

What BEST DESCRIBES a positively charged ion?

a)

Proton

b)

Atom

c)

Anion

d)

Cation

27.

Valence electrons are easier to remove when there are more inner shell electrons to weaken the attraction of the nucleus. This is called....

a)

Valence Electron Protection

b)

Electron Shielding

c)

Ionization Energy

d)

Electron Affinity

28.

The distance between the center of the nucleus to the outer boundary of the highest energy level electron cloud is defined as...

a)

Atomic Radius

b)

Atomic Mass

c)

Atomic Number

d)

Electronegativity

29.

What best describes electronegativity?

a)

The shielding of valence electrons from the nucleus by inner shell electrons

b)

The amount of energy needed to remove an electron from an atom.

c)

The amount of energy released when an electron is added to an atom.

d)

A chemical property of an atom to attract electrons while bonded in a compound.

30.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

31.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

32.
Which periodic table family could have electrons filling orbitals in the s-block?
a)
Alkaine Earth 
b)
Halogens
c)
Noble Gases
d)
Transition Metals
33.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
34.

What color of light has the greatest energy per photon?

a)

Red

b)

Green

c)

Blue

d)

Violet

35.

Which of the jumps in energy levels would create a photon emission with the most energy?

a)

n=1 to n=2

b)

n=2 to n=3

c)

n=2 to n=4

d)

n=1 to n=4

36.

This image shows some of the colored flames we will see in the fire lab. The color of light can show us which emission has the most energy released by the electrons. Which compound's electrons had the largest change in energy levels?

a)

Strontium

b)

Calcium

c)

Potassium

d)

Copper

37.

The frequency of violet light is 7.5x1014 Hz. What is its wavelength?

a)

4.0x10-7 m

b)

4.0x107 m

c)

2.25x1023m

d)

2.25x1023 Hz

38.
Violet light has a wavelength of
4.10 x 10-12  m. What is the frequency?
a)
1.23 x 10^ -3 Hz
b)
7.31 x 10^ 19 Hz
c)
1.37 x 10^12 Hz
d)
3.0 x 10^ 8 Hz
39.

Calculate the wavelength of blue light emitted by a mercury lamp with a frequency of 6.88 x 1014 Hz.

a)

3.44 x 10-6m

b)

4.36 x 10-7m

c)

3.0 x 108 m

d)

633 m

40.

What is the frequency of a photon whose energy is 3.4x10-19J? (h= 6.626x 10^-34 Js)

a)

8.8x1026 Hz

b)

5.1x1014 Hz

c)

1.9x10-15 Hz

d)

2.3x10-52 Hz

41.

When an electron in the _______state absorbs energy, it goes to the ________ state.

a)

lower, excited

b)

ground state, higher state

c)

ground state, excited state

d)

excited state, ground state

42.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
43.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
44.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
45.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
46.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
47.
1.  What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
48.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
49.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
50.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
51.

Each orbital has at most two electrons that spin in opposite directions.

a)

Pauli exclusion principle

b)

aufbau principle

c)

electron configuration

d)

Hund's rule

52.

Which of the following states that a single electron occupies each orbital within a subshell before electrons begin pairing?

a)

Hund's rule

b)

aufbau principle

c)

pauli exclusion principle

d)

lewis rule

53.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
54.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
55.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
56.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
57.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
58.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
59.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
60.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

61.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

62.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

63.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

64.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

65.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

gold + oxygen

66.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

67.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

68.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

69.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

70.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

71.
Name this compound: 
KF
a)
Potassium fluoride
b)
Potassium fluorite
c)
Fluorine potasside 
d)
Potassium fluorate
72.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
73.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
74.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
75.
What is the chemical formula for Nitrogen triiodide?
a)
NI
b)
N3I
c)
NI3
d)
None of these
76.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
77.
What is the chemical formula for CP ?
a)
Carbon phosphide
b)
Monocarbon phosphide
c)
Carbon monophosphide
d)
none of the above
78.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
79.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
80.
What's the formula for chlorine dioxide
a)
ClO2
b)
CLO
c)
ClO3
d)
HClO2
81.
What is the formula for Hexaboron Monosilicide
a)
B6Si
b)
BSi
c)
BSi6
d)
B6Si6
82.

Write the formula: iodine heptafluoride

a)

IF7

b)

I2F14

c)

IHF7

d)

IF6

83.

Name the following: C3H8

a)

Tricarbon octahydride

b)

Carbon hydride

c)

Carbon octahydride

d)

Tricarbon hydride

84.
An ionic compound of calcium and chlorine would be named
a)
calcium chlorine.
b)
calcium chlorite.
c)
calcium chloride.
d)
chlorine calcium.

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