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chemistry test prep

Total questions: 80

Worksheet time: 43mins

Name
Class
Date
1.

The speed of a wave indicates how fast a given peak travels through water

a)

True

b)

False

2.

The frequency of the wave indicates how many wave peaks pass a certain point per given time period

a)

True

b)

False

3.

Which colour of visible light has the most energy per proton?

a)

Violet

b)

Blue

c)

Green

d)

Yellow

4.

When an electron in the ground state absorbs energy, it goes to a(n)_____state

a)

excited

b)

lower

c)

frenetic

d)

ionic

e)

stable

5.

The energy levels of the hydrogen atom (and all atoms) are _____, meaning that only certain discrete energy levels are allowed.

a)

varied

b)

quantized

c)

ramp-like

d)

continuous

e)

two of these

6.

The probability map for an electron is called

a)

an orbitq

b)

a photon

c)

an orbital

d)

an electron configuration

e)

none of these

7.

As the principal energy level increases In an atoms orbitals, the average distance of an electron energy level from the nucleus _____

a)

increases

b)

decreases

c)

stays the same

d)

varies

e)

none of these

8.

A given set of F orbitals consists of _____ orbitals

a)

1

b)

3

c)

5

d)

7

e)

9

9.

The maximum number of electrons allowed in each of the P orbitals is

a)

2

b)

4

c)

8

d)

18

e)

none of these

10.

A given set of D orbitals consists of _____ orbitals

a)

1

b)

3

c)

5

d)

6

e)

none

11.

The maximum number of electrons allowed in each of the d orbitals is

a)

2

b)

4

c)

8

d)

18

e)

32

12.

A d sub level can hold a maximum of _____ electrons

a)

5 electrons

b)

10 electrons

c)

14 electrons

d)

32 electrons

e)

none of these

13.

The elements chlorine and iodine have similar chemical properties because they

a)

a. are both metals and can easily lose electrons to form compounds

b)

b. are in the same chemical period

c)

c. have the same number of electrons in their outer energy levels

d)

d. have the same number of stable isotopes

e)

e. none

14.

The alkaline earth metals have how many valence electrons?

a)

8

b)

7

c)

3

d)

2

e)

1

15.

The noble gases contain how many valence electrons?

a)

1

b)

7

c)

0

d)

8

e)

none

16.

All of these atoms have seven electrons in their outermost energy levels EXCEPT _____

a)

H

b)

F

c)

Cl

d)

Br

e)

I

17.

The maximum number of electrons in the second principal energy level of an atom is _____

a)

2

b)

6

c)

8

d)

18

e)

32

18.

Which element has the fewest electrons in its valence shell?

a)

Cs

b)

Mg

c)

p

d)

O

e)

Br

19.

Which one of the following atoms has a partly filled d sub level?

a)

Ca

b)

Ni

c)

Zn

d)

As

e)

Ar

20.

What is the maximum number of electrons that a given orbital can hold?

a)

10

b)

6

c)

5

d)

4

e)

2

21.

Which of the following statements is true of 1s orbital of krypton?

a)

It is smaller then the helium 1s orbital because krypton's p and d orbitals crowd the s orbitals

b)

It is larger then the helium 1s orbital because krypton contains more electrons

c)

It is smaller then the helium 1s orbital because kryptons nuclear charge draws the electrons closer

d)

It is the same size as that of the helium 1s orbital because both s orbitals can only have 2 electrons

e)

It is larger then the helium 1s orbital because kryptons ionization energy is lower so its easier to remove electrons

22.

Which of the following atoms has the smallest atomic radius?

a)

As

b)

Sb

c)

Bi

d)

P

e)

N

23.

Which of the following has the smallest atomic radius?

a)

N

b)

F

c)

Br

d)

Cl

e)

S

24.

Which of the following statements is correct and provides the best explanation for what happens when the first two electrons are removed from calcium?

a)

Energy is released when either electron comes off since calcium is a metal and not very electronegative

b)

It takes less energy to remove the second electron from calcium as compared to the first because calcium wants to have 8 electrons in its outer shell (and have a noble gas configuration)

c)

It takes less energy to remove the first electron as compared to the second because it is in a higher energy level than the second electron

d)

It takes more energy to remove the second electron as compared to the first because the nucleus binds the electrons more tightly as each electron is removed

e)

Electrons cannot be removed from calcium since it is a metal and only wants to gain electrons to become more stable

25.

Which of the following elements of group 1A has the highest ionization energy?

a)

Li

b)

K

c)

Rb

d)

Na

e)

Cs

26.

Order the elements Al, Cl, and F in terms of increasing atomic radius

a)

F, Al, Cl

b)

F, Cl, Al

c)

Al, Cl, F

d)

Al, F, Cl

e)

Cl, Al, F

27.

Which has the highest ionization energy, K or Br?

(a)  

28.

Which of the following statements about the periodic table is FALSE

a)

Elements in the same column have similar reactivities because their valence electrons tend to be located in the same type of orbitals

b)

A Series of ions that are isoelectronic must have the same electron configuration

c)

The atomic size of the elements increases going across a period from left to right because the number of electrons increases, so they are located further from the nucleus

d)

It takes more energy to remove an electron from lithium than from cesium because the valence electrons in lithium are located closer to the nucleus

e)

Fluorine is the most electronegative element due to its size and nuclear charge

29.

How does magnesium compare with sodium in terms of the following properties?

a) atomic size

b) number of outer shell electrons

c) ionization energy

d) Formula of the bromide salt

(a)  

30.

An atom has a valence shell electron configuration of ns1. TO which group of metals in the periodic table does it belong?

a)

a. Alkali Metals

b)

b. Alkaline Earth Metals

c)

c. Halogens

d)

d. Noble Gases

e)

e. Inner transition metals

31.

An atom has a valence shell electron configuration of ns2. To which group of metals in the periodic table does it belong?

a)

Alkali Metals

b)

alkaline earth metals

c)

halogen

d)

noble gases

e)

inner transition metals

32.

An atom has a valence shell electron configuration of ns2np5. To which group of metals in the periodic table does it belong?

a)

alkali metals

b)

alkaline earth metals

c)

halog

d)

noble gases

e)

inner transition metals

33.

Going down the periodic table, in a group of non-metals, which property decreases in value?

a)

Reactivity

b)

Atomic Num

c)

Atomic R

d)

Density

e)

Number of Isotopes

34.

Going down the periodic table in a group of metals, which property decreases in value?

a)

Reactivity

b)

Atomic Number

c)

Atomic Radius

d)

Density

e)

Ionization Energy

35.

A bond is a force that holds groups of two or more atoms together and makes them function as a unit

a)

True

b)

False

36.

Covalent bonding occurs when electrons are shared by nuclei

a)

True

b)

False

37.

The greater the difference in electronegativity between two bonded atoms, the more polar the bond

a)

T

b)

False

38.

In general, a larger atom has a smaller electronegativity

a)

True

b)

False

39.

In ionic bonding

a)

The electrons are shared between the atoms

b)

The process of forming an ionic bond is highly endo

c)

the bonding that occurs is usually between two nonmetal atoms

d)

a noble gas configuration is formed for each element or ion

e)

At least two of the above statements are correct

40.

N2 is an example of a covalent bond

a)

T

b)

False

41.

Which of the following statements are true?

I. The electrons in each molecule tend to be attracted to the most electronegative element

II. Each molecular drawing follows the localized electron model

III. Both HF and CO2 are linear molecules and therefore non-polar

IV. The bond angles of NH3 are slightly less then 109.5 degrees because the lone pair compresses the angles between the bonding pairs

a)

I, III, IV

b)

I, II, IV

c)

I, II, III

d)

II, IV

e)

All of the above statements (I-IV) are correct

42.

True or False? CH4 has ionic bonds

a)

T

b)

False

43.

Is the molecule CO2 ionic or covalent?

a)

Ionic

b)

Covalent

44.

Would K2O be classified as ionic or covalent?

a)

Ionic

b)

Covalent

45.

Would MgCl2 be classified as ionic or covalent?

a)

Ionic

b)

Covalent

46.

Would NaBr be classified as ionic or covalent?

a)

Ionic

b)

Covalent

47.

Would NH3 be classified as ionic or covalent?

a)

Ionic

b)

Covalent

48.

Would CoCl2 be classified as ionic or covalent?

a)

Ionic

b)

Covalent

49.

Would CH4 be classified as Ionic or Covalent

a)

Ionic

b)

Covalent

50.

Would SF4 be classified as ionic or covalent

a)

Ionic

b)

Covalent

51.

Would AlCl3 be classified as ionic or covalent

a)

Ionic

b)

Covalent

52.

Is the molecule CF4 non polar or Polar?

a)

Polar

b)

Nonpolar

53.

Is the molecule H2S non polar or polar?

a)

Polar

b)

Nonpolar

54.

Which of the following compounds contains an ionic bond

a)

HCl(g)

b)

NaCl

c)

CCl4

d)

SO2

55.

Which of the following compounds contains one or more covalent bonds?

a)

SO2

b)

NaBr

c)

Rb2O

d)

MgBr2

e)

MgO

56.

Which of the following elements is the most electronegative element?

a)

C

b)

Ge

c)

Pb

d)

Si

57.

The most electronegative element of those listed is

a)

Zn

b)

Si

c)

Sr

d)

Ba

e)

Zr

58.

The least electronegative element of those listed is

a)

O

b)

P

c)

Ba

d)

Cu

e)

Se

59.

Which of the following elements has the lowest electronegativity?

a)

Cs

b)

Na

c)

Be

d)

Se

60.

Which of the following contains only non polar bonds?

a)

CH4

b)

HCl

c)

H2O

d)

Mg3N2

e)

Cl2

61.

Which of the following molecules has only non polar covalent bonds?

a)

N2

b)

CO

c)

HI

d)

CCl4

e)

NaCl

62.

The number of polar covalent bonds in SF4 is

a)

4

b)

3

c)

1

d)

2

e)

none

63.

If atom X Forms a diatomic molecule with itself, the bond is

a)

ionic

b)

polar covalent

c)

non polar covalent

d)

polar coordinate covalent

e)

none

64.

Arrange the following elements in order of their increasing electronegativity

a)

Be < C < N < F

b)

C < N < F < Be

c)

N < C < Be < F

d)

C < F < Be < N

e)

F < N < C <Be

65.

Which of the following bonds does not have a dipole moment?

a)

H-H

b)

B-H

c)

N-H

d)

Li-H

e)

S-H

66.

When a molecule has a centre of positive charge and a centre of negative charge, it is said to have a

a)

magnetic attraction

b)

diatomic

c)

double bond

d)

polyatomic ion

e)

dipole moment

67.

One of the most important characteristics of the water molecule is its _____, which allows it to surround and attract both positive and negative ions

a)

polarity

b)

strength

c)

magnetism

d)

fluidity

e)

stability

68.

True or False? The F- and O2- ions have the same electron configuration

a)

True

b)

False

69.

Magnesium reacts with Oxygen to form

a)

MgO

b)

MgO2

c)

Mg2O

d)

Mg2O3

e)

none

70.

Strontium reacts with chlorine to form

a)

SrCl2

b)

SrCl

c)

Sr2Cl

d)

Sr2Cl3

e)

none

71.

When they react chemically, the alkali metals (Group 1 A)

a)

Gain 1 electron

b)

Gain 7 electrons

c)

gain or lose 7 electrons

d)

lose 1 electron

72.

The formula of the compound formed after the reaction between lithium and oxygen is

a)

Li2O

b)

LiO2

c)

Li2O3

d)

LiO

e)

none

73.

An oxygen atom needs to gain ____ electrons to achieve a noble gas configuration

a)

2

b)

1

c)

3

d)

4

e)

5

74.

Which of the following has a double bond?

a)

H2O

b)

NH3

c)

O2

d)

CO

e)

H2S

75.

Which has a planar structure?

a)

SO32-

b)

CO32-

c)

NF3

d)

H3O+

e)

CH4

76.

Which has a tetrahedral structure

a)

SO32-

b)

CO32-

c)

SO3

d)

NH3

e)

CH4

77.

Which has a bent structure?

a)

O

b)

CO2

c)

H2O

d)

NH3

e)

CaCl2

78.

Which of the following has the largest radius?

a)

S

b)

Cl

c)

Ar

d)

K

e)

Ca

79.

Which of the following has the smallest radius

a)

S

b)

Cl

c)

Ar

d)

K

e)

Ca

80.

The frequency of the wave is the distance between two consecutive wave peaks

a)

true

b)

false

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