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IB Chemistry SL/HL1 Topic 2 Multiple Choice Review

Total questions: 75

Worksheet time: 19hrs 45mins

Name
Class
Date
1.

Consider the composition of each species below. Which is an anion?

a)

9 protons, 10 neutrons, 10 electrons

b)

11 protons, 12 neutrons, 11 electrons

c)

12 protons, 12 neutrons, 12 electrons

d)

13 protons, 14 neutrons, 10 electrons

2.

Energy levels for an electron in a hydrogen atom are

a)

evenly spaced.

b)

farther apart near the nucleus.

c)

closer together near the nucleus.

d)

arranged randomly.

3.

Which is related to the number of electrons in the outer main energy level of the elements from the alkali metals to the halogens?

I. Group number

II. Period number

a)

I only

b)

II only

c)

Both I and II

d)

Neither I nor II

4.

How do bond length and bond strength change as the number of bonds between two atoms increases?

a)

Bond length increases, Bond strength increases

b)

Bond length increases, Bond strength decreases

c)

Bond length decreases, Bond strength increases

d)

Bond length decreases, Bond strength decreases

5.

Which of the following is true for CO2?

a)

C=O bond polar; CO2 molecule non-polar

b)

C=O bond non-polar; CO2 molecule polar

c)

C=O bond polar; CO2 molecule polar

d)

C=O bond non-polar; CO2 molecule non-polar

6.

The molar masses of C2H6, CH3OH and CH3F are very similar. How do their boiling points compare?

a)

C2H6 < CH3OH < CH3F

b)

CH3F < CH3OH < C2H6

c)

CH3OH < CH3F < C2H6

d)

C2H6 < CH3F < CH3OH

7.

What is the correct number of each particle in a fluoride ion, 19F– ?

a)

protons 9, neutrons 10, electrons 8

b)

protons 9, neutrons 10, electrons 9

c)

protons 9, neutrons 10, electrons 10

d)

protons 9, neutrons 19, electrons 10

8.

Which statement is correct for the emission spectrum of the hydrogen atom?

a)

The lines converge at lower energies.

b)

The lines are produced when electrons move from lower to higher energy levels.

c)

The lines in the visible region involve electron transitions into the energy level closest to the nucleus.

d)

The line corresponding to the greatest emission of energy is in the ultraviolet region.

9.

How many valence electrons are present in an atom of an element with atomic number 16?

a)

2

b)

4

c)

6

d)

8

10.

A certain sample of element Z contains 60% of 69Z and 40% of 71Z. What is the relative atomic mass of element Z in this sample? Round to 3 sig figs and use ONLY THE NUMBERS, NO UNITS

(a)  

11.

What is the difference between two neutral atoms represented by the symbols 5927 Co and 5928Ni?

a)

The number of neutrons only.

b)

The number of protons and electrons only.

c)

The number of protons and neutrons only.

d)

The number of protons, neutrons and electrons.

12.

How many electrons are there in one 2412 Mg2+ ion?

a)

10

b)

12

c)

14

d)

22

13.

The electron arrangement of sodium is 2.8.1. How many occupied main electron energy levels are there in an atom of sodium?

a)

1

b)

3

c)

10

d)

11

14.

Information about 4 different atoms is given in the chart. Which two atoms are isotopes?

a)

W and Y

b)

W and Z

c)

X and Z

d)

X and Y

15.

Which statement is correct about a line emission spectrum?

a)

Electrons absorb energy as they move from low to high energy levels.

b)

Electrons absorb energy as they move from high to low energy levels.

c)

Electrons release energy as they move from low to high energy levels.

d)

Electrons release energy as they move from high to low energy levels.

16.

How many neutrons are there in the ion 18O2–?

a)

8

b)

10

c)

16

d)

20

17.

What is the electron arrangement of silicon?

a)

2.4

b)

2.8

c)

2.8.4

d)

2.8.8

18.

Which statement is correct about the isotopes of an element?

a)

They have the same mass number

b)

They have the same electron arrangement

c)

They have more protons than neutrons

d)

They have the same numbers of protons and neutrons

19.

What is the difference between two neutral atoms represented by the symbols 21084Po and 21085At?

a)

The number of neutrons only.

b)

The number of protons and electrons only.

c)

The number of protons and neutrons only.

d)

The number of protons, neutrons and electrons.

20.

Which statements are correct for the emission spectrum of the hydrogen atom? Select all that apply.

a)

The lines converge at lower energies.

b)

Electron transition to n =1 are responsible for lines in the UV region.

c)

Lines are produced when electrons move from higher to lower energy levels.

21.

What is the symbol for a species that contains 15 protons, 16 neutrons and 18 electrons?

a)

3116S

b)

3116S3-

c)

3115P-

d)

3115P3-

22.

What is the electron arrangement of an Al3+ ion?

a)

2, 8

b)

2, 3

c)

2, 8, 3

d)

2, 8, 8

23.

Which species has 54 electrons and 52 protons?

a)

12852Te2-

b)

13254Xe2+

c)

13254Xe2-

d)

12852Te2+

24.

What is the correct sequence for the processes occurring in a mass spectrometer?

a)

vaporization, ionization, acceleration, deflection

b)

vaporization, acceleration, ionization, deflection

c)

ionization, vaporization, acceleration, deflection

d)

ionization, vaporization, deflection, acceleration

25.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
26.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
27.
What is the electron configuration of Sulfur  using noble gas method
a)
[Ne]3s1
b)
[Ne]3s23p3
c)
[Ne]3s23p4
28.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
29.

There are __ energy levels

a)

1

b)

2

c)

7

d)

8

30.
How many atomic orbitals are there in the p sublevel?
a)
2
b)
3
c)
4
d)
5
31.
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
32.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
33.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
c)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
34.
What does Hund's rule states ?
a)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
35.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
36.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
37.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
38.
How many electron can be found in a s orbital?
a)
2
b)
3
c)
4
d)
1
39.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
40.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
41.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
42.

The second energy level contains...

a)

s and p orbitals

b)

s orbitals only

c)

s, p, d and f orbitals

d)

s, p, and d orbitals

43.
Which of the waves shown below has the higher frequency?
a)
wave A
b)
Wave B
44.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
45.

Which electron configuration belongs to a Chloride (Cl-) ion?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

d)

1s2 2s2 2p6 3p7

46.
What electron configuration matches an oxygen ion?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
47.

Write the electronic structure for Cu+1 ion

a)

[Ar]4s13d10

b)

[Ar]4s13d9

c)

[Ar]4s03d10

d)

[Ar]3d10

48.

Write the electronic structure for Mn4+ ion

a)

[Ar]4s23d5

b)

[Ar]4s23d1

c)

[Ar]4s03d2

d)

[Ar]3d3

49.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
50.

Which element ends 4p4?

a)

sulfur

b)

arsenic

c)

selenium

d)

antimony

51.

What is the state when electrons move to a higher energy level upon absorption of energy?

a)

active

b)

inactive

c)

excited

d)

ground

52.

What particles in the heated compounds are responsible for the production of the colored light?

a)

proton

b)

neutron

c)

electron

d)

proton and neutron

53.

Which is the electron configuration of an aluminum atom (13Al) in the excited state?

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3p2

c)

1s2 2s2 2p6 3s2 4s1

d)

1s2 2s2 2p6 3s2 3p3

54.

When heated, electrons are ____________.

a)

annoyed

b)

irritated

c)

excited

d)

angered

55.
If electrons gain energy they 
a)
move up one or more shells
b)
more down one or more shells
56.

What type of ions do metals form?

a)

cations

b)

anions

57.

What types of ions do nonmetals form?

a)

cations

b)

anions

58.

Which of the following would pairs would give the same flame test results?

a)

NaCl & MgCl2

b)

LiCl & LiBr

c)

CaCO3 and MgCO3

d)

H2O and HCl

59.

What evidence did you observe that proves that elements give off their own unique color spectrum?

a)

All of the gas tubes produced a full spectrum. (A rainbow.)

b)

When we looked at white light through a prism, we saw the rainbow.

c)

Each gas tube gave off its own unique color and color spectrum when we looked at the light through the spectroscope. None of them were the exact same.

d)

Each gas tube gave off the same color and color spectrum when we looked at the light through a spectroscope.

60.

Regardless of how hot the flame is, when a metal ion is placed in a flame, it always give off the same color light. Why?

a)

The number of protons is still the same, so the same number of electrons get excited and fall back to the ground state the same way and give off the same color every time.

b)

The number of electrons is still the same, so the same number of electrons get excited and fall back to the ground state the same way and give off the same color every time.

c)

The number of neutrons is still the same, so the same number of electrons get excited and fall back to the ground state the same way and give off the same color every time.

d)

The number of ions is still the same, so the same number of electrons get excited and fall back to the ground state the same way and give off the same color every time.

61.

The common isotopes of hydrogen have masses of 1 amu, 2 amu, and 3 amu. The average atomic mass of hydrogen is 1.00794 amu. This shows that the most common isotope has a mass of

a)

1 amu

b)

2 amu

c)

3 amu

d)

4 amu

62.

A new element, unbiennium, has been synthesized. A typical sample contains 22.50 percent Ube–323 and 77.50 percent Ube–325. What is the average mass?

a)

324.6 amu

b)

323.4 amu

c)

324.0 amu

d)

325.2 amu

63.

Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37, The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant?

a)

Cl-35

b)

Cl-37

c)

Cannot be determined from the information provided.

64.

The box for an element from the periodic table is shown. Which is the atomic mass?

a)

A

b)

B

c)

C

d)

D

65.

An element has three isotopes. Given the abundances and relative masses, calculate the average atomic mass and determine (from the periodic table) which element it is.


Abundances | Relative masses

0.005% | 234.04 amu

0.720% | 235.04 amu

99.275% | 238.05 amu

a)

Uranium (#92, Atomic Mass: 238.03 amu)

b)

Fluorine (#9, Atomic Mass: 19.00 amu)

c)

Mercury (#89, Atomic Mass: 200.59 amu)

d)

Polonium (#84 209 amu)

66.

If the masses of one isotope of nitrogen, nitrogen-14, is 14.003 amu and another isotope, nitrogen-15, is 15.000 amu, find the relative abundance of the isotopes. Select all that are true.

a)

nitrogen-14 is 99.6%

b)

nitrogen-15 is 0.4%

c)

nitrogen-15 is 99.6%

d)

nitrogen-14 is 0.4%

e)

Both are 50% since there are only 2 isotopes

67.
Which species would get deflected by the greatest degree in the mass spectrometer?
a)
12C+
b)
13C+
c)
13C2+
d)
14C+
68.
What do the peaks on the mass spectrum represent?
a)
anions
b)
different isotopes
c)
atoms with differing numbers of electrons
d)
numbers of electrons
69.
Which element does this mass spectrum most likely represent?
a)
neon
b)
scandium
c)
boron
d)
sodium
70.
What do you expect the molar mass to be for this element?
a)
91.4 g/mol
b)
90.0 g/mol
c)
4 g/mol
d)
50. g/mol
71.

The arrows pointing down represents...

a)

photon absorption

b)

proton emission

c)

electron absorption

d)

photon emission

72.

As the energy level increases the difference in the energy level ...

a)

increases

b)

decreases

c)

stays the same

d)

none of these

73.
When an atom has all of its electrons in the lowest energy orbitals available, the atom is  
a)
in ground state
b)
in excited state
c)
giving off light energy
d)
unstable
74.
The _______________ determines the color of visible light. 
a)
wavelength
b)
speed
c)
amplitude
d)
light
75.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low

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