Free Printable CHEM 01 - Summative Test 2

1.

The effective nuclear charge of an atom is primarily affected by _________.

a)

inner electrons

b)

outer electrons

c)

nuclear charge

d)

electron distribution

e)

orbital radial probability

2.

The type of compound that is most likely to contain a covalent bond is __________.

a)

one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table.

b)

a solid metal.

c)

one that is composed of only nonmetals.

d)

held together by the electrostatic forces between oppositely charged ions

e)

There is no general rule to predict covalency in bonds.

3.

The basis of the VSEPR model of molecular bonding is ______.

a)

regions of electron density on an atom will organize themselves so as to maximize s-character

b)

regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap

c)

atomic orbitals of the bonding atoms must overlap for a bond to form

d)

electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions

e)

hybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetry

4.

Of the reactions below, which one is a decomposition reaction?

a)

$NH_4Cl\ \rightarrow\ NH_{3_{ }}+HCl$

b)

$2Mg\ +O_2\ \rightarrow\ 2MgO$

c)

$2N_2+3H_2\ \rightarrow\ 2NH_3$

d)

$2CH_4+4O_2\ \rightarrow\ 2CO_2+4H_2O$

e)

$Cd\left(NO_3\right)_2+Na_2S\ \rightarrow CdS\ +2NaNO_3$

5.

Atomic radius generally increases as we move ______.

a)

down a group and from right to left across a period

b)

up a group and from left to right across a period

c)

down a group and from left to right across a period

d)

up a group and from right to left across a period

e)

down a group; the period position has no effect

6.

As the number of covalent bonds between two atoms increases, the distance between the atoms _____ and the strength of the bond between them ________.

a)

increases, increases

b)

decreases, decreases

c)

increases, decreases

d)

decreases, increases

e)

is unpredictable, is unpredictable

7.

The chemical formula of nitrobenzene is

C_6H_5NO_2

. The molecular weight of this compound is ______ amu.

a)

107.11

b)

43.03

c)

109.10

d)

123.11

e)

3.06

8.

The percentage (%) composition by mass of F in the binary compound $KrF_2$ is _____.

a)

18.48

b)

45.38

c)

68.80

d)

81.52

e)

31.20

9.

Of the following elements, ______ has the most negative electron affinity.

a)

S

b)

Cl

c)

Se

d)

Br

e)

I

10.

Sodium is much more apt to exist as a cation than is chlorine. This is because ______.

a)

chlorine is a gas and sodium is a solid

b)

chlorine has a greater electron affinity than sodium does

c)

chlorine is bigger than sodium

d)

chlorine has a greater ionization energy than sodium does

e)

chlorine is more metallic than sodium

11.

In counting the electron domains around the central atom in VSEPR theory, a ________ is not included.

a)

nonbonding pair of electrons

b)

single covalent bond

c)

core level electron pair

d)

double covalent bond

e)

triple covalent bond

12.

Of the following species, _____ will have bond angles of $120^{\degree}$ .

a)

$PH_3$

b)

$ClF_3$

c)

$NCl_3$

d)

$BCl_3$

e)

All of these will have bond angles of $120\degree$

13.

A 30.5 gram sample of glucose ( $C_6H_{12}O_6$ ) contains ______ mol of glucose.

a)

0.424

b)

0.169

c)

5.90

d)

2.36

e)

0.136

14.

A sample of $CH_4O$ with a mass of 32.0 g contains _____ molecules $CH_4O$ .

a)

$5.32\ \times10^{-23}$

b)

1.00

c)

$1.88\ \times10^{22}$

d)

$6.02\ \times10^{23}$

e)

32.0

15.

Elements in the modern version of the periodic table are arranged in order of increasing ___________.

a)

oxidation number

b)

atomic mass

c)

average atomic mass

d)

atomic number

e)

number of isotopes

16.

Which of the following are combustion reactions?

i.

CH_4\ +\ O_2\ \rightarrow\ CO_2+H_2O

ii.

CaO\ +\ CO_2\ \rightarrow CaCO_3

iii.

PbCO_3\ \rightarrow\ PbO\ +\ CO_2

iv.

CH_3OH\ +O_2\ \rightarrow\ CO_2\ +H_2O

a)

i and iv

b)

i, ii, iii and iv

c)

i, iii and iv

d)

ii, iii and iv

e)

iii and iv

17.

Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar?

a)

Mg > Na > P > Si > Ar

b)

Ar > Si > P > Na > Mg

c)

Si > P > Ar > Na > Mg

d)

Na > Mg > Si > P > Ar

e)

Ar > P > Si > Mg > Na

18.

Of the molecules below, only ______ is polar

a)

$CCl_4$

b)

$CH_4$

c)

$SeF_4$

d)

$SiCl_4$

19.

The molecular geometry of the $PF_3$ molecule is ________ and this molecule is _________.

a)

trigonal planar, polar

b)

trigonal planar, nonpolar

c)

trigonal pyramidal, polar

d)

trigonal pyramidal, nonpolar

e)

tetrahedral, unipolar

20.

The molecular geometry of $BeCl_2$ molecule is ______ and this molecule is ________.

a)

bent, nonpolar

b)

linear, polar

c)

bent, polar

d)

seesaw, polar

e)

linear, nonpolar

21.

Of the molecules below, the bond in ______ is the most polar.

a)

$HBr$

b)

$HI$

c)

$HCl$

d)

$HF$

e)

$H_2$

22.

How many electrons are in the Lewis structure of a nitrite $\left(NO_2\ ^-\right)$ ion?

a)

18

b)

17

c)

16

d)

23

e)

24

23.

Based on the octet rule, boron will most likely form a ______ ion.

a)

$B^{3-}$

b)

$B^{3+}$

c)

$B^+$

d)

$B^{2+}$

e)

$B^{2-}$

24.

Which of the following does not have eight (8) valence electrons?

a)

$Cl^-$

b)

$Xe$

c)

$Ti^{+4}$

d)

$Rb^+$

e)

$Sr^+$

25.

Of the possible bonds between carbon atoms (single, double, and triple), ________.

a)

a triple bond is longer than a single bond

b)

a double bond is stronger than a triple bond

c)

a single bond is stronger than a triple bond

d)

a double bond is longer than a triple bond

e)

a single bond is stronger than a double bond

26.

The electron configuration of phosphide $\left(P^{3-}\right)$ ion is ____.

a)

$\left[Ne\right]3s^2$

b)

$\left[Ne\right]3s^23p^1$

c)

$\left[Ne\right]3s^23p^3$

d)

$\left[Ne\right]3p^2$

e)

$\left[Ne\right]3s^23p^6$

27.

The halogens, alkali metals, and alkaline earth metals have _______ valence electrons, respectively.

a)

7, 4 and 6

b)

1, 5 and 7

c)

8, 2 and 3

d)

7, 1 and 2

e)

2, 7 and 4

28.

Which isoelectronic series is correctly arranged in order of increasing radius?

a)

$K^+\ <\ Ca^{2+}\ <\ Ar\ <Cl^-$

b)

$Cl^-\ <Ar\ <\ K^+\ <Ca^{2+}$

c)

$Ca^{2+}\ <Ar\ <\ K^+\ <Cl^-$

d)

$Ca^2+\ <\ K^+\ <\ Ar\ <Cl^-$

e)

$Ca^{2+\ }<\ K^+\ <Cl^-\ <Ar$

29.

Rank the following in terms of DECREASING first ionization energies:

a)

Ne > O > N > Be > B

b)

Ne > N > O > B > Be

c)

Ne > O > N > B > Be

d)

Ne > N > O > Be > B

e)

B > Be > O > N > Ne

30.

Which ion below has the LARGEST radius?

a)

$Cl^-$

b)

$K^+$

c)

$Br^-$

d)

$F^-$

e)

$Na^+$

31.

Which of the following species has the smallest ionic radius?

a)

$Al^{3+}$

b)

$Na^+$

c)

$Mg^{2+}$

d)

$S^{2-}$

e)

$Cl^-$

32.

Of the following elements, _________ has the most negative electron affinity.

a)

P

b)

Al

c)

Si

d)

Cl

e)

B

33.

The reason bromine is more likely to exist as an anion than is potassium is because _______.

a)

bromine is bigger than potassium

b)

bromine has a greater ionization energy than potassium does

c)

bromine has a greater electron affinity than potassium does

d)

bromine is a liquid and potassium is a solid

e)

bromine is more metallic than potassium

34.

All of the following are ionic compounds except ________.

a)

$CH_4$

b)

$K_2O$

c)

$Be\left(OH\right)_2$

d)

$NiCl_2$

e)

$Sr_3N_2$

35.

Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)?

a)

Ge < Si < S < O < Ne

b)

Ne < O < S < Si < Ge

c)

Ne < S < O < Si < Ge

d)

Ne < Si < O < S < Ge

e)

Ne < Ge < Si < S < O

36.

________ is isoelectronic with krypton.

a)

$Se^{2-}$

b)

$Se^{3-}$

c)

$Br$

d)

$Se^{2+}$

e)

$Te^{2-}$

37.

_________ is isoelectronic with argon.

a)

$Cl^-$

b)

$P^{4-}$

c)

$Ca$

d)

$K^-$

e)

$F^-$

38.

Which element would be expected to have chemical and physical properties closest to those of rubidium?

a)

Cu

b)

Fe

c)

S

d)

Ca

e)

K

39.

An electron domain is _______.

a. nonbonding pair of electrons

b. single bond

c. multiple bond

a)

a only

b)

b only

c)

c only

d)

a, b and c

e)

b and c

40.

When the following equation is balanced, the coefficients are ______.

C_8H_{18}\ +\ O_2\ \rightarrow\ CO_2\ +\ H_2O

a)

2, 3, 4, 4

b)

1, 4, 8, 9

c)

2, 12, 8, 9

d)

4, 4, 32, 36

e)

2, 25, 16, 18

41.

There are ______ mol of carbon atoms in 4 mol of

C_4H_8O_2

.

a)

4

b)

8

c)

16

d)

20

e)

32

42.

How many moles of pyridine ( $C_5H_5N$ ) are contained in 4.14 g of pyridine?

a)

0.0523

b)

327

c)

$6.88\ \times10^{-24}$

d)

$2.49\ \times10^{24}$

e)

79.1

43.

The combustion of propane ( $C_3H_8$ ) produces $CO_2$ and $H_2O$ .

C_3H_8\ +5O_{2\ }\rightarrow\ 3CO_2\ +4H_2O

The reaction of 2.5 mol of

O_2

will produce ______ mol of

H_2O

.

a)

4.0

b)

3.0

c)

2.5

d)

2.0

e)

1.0

44.

When the following equation is balanced, the coefficient of $H_2S$ is __________.

FeCl_3\ +\ H_2S\ \rightarrow\ Fe_2S_3\ +HCl

a)

1

b)

2

c)

3

d)

5

e)

4

45.

Calculate the percentage by mass of lead (Pb) in $Pb\left(NO_3\right)_2$ .

a)

38.6

b)

44.5

c)

62.6

d)

65.3

e)

71.2

CHEM 01 - Summative Test 2 - Block O

Total questions: 45

Worksheet time: 1hrs 28mins

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