Free Printable Chem exam 2

1.

How many valence electrons in C (Carbon) atom?

a)

1

b)

2

c)

3

d)

4

e)

5

2.

give the number of lone pairs around the central atom and the molecular geometry of CBr4

a)

0 lone pairs, square planar

b)

0 lone pairs, tetahedral

c)

1 lone pair, square pyramidal

d)

1 lone pair, trigonal bipyramidal

3.

Give the number of lone pairs around the central atom and the molecular geometry of XeF2

a)

0 lone pairs, linear

b)

1 lone pair, bent

c)

2 lone pairs, bent

d)

3 lone pairs, bent

e)

3 lone pairs, linear

4.

give the number of lone pairs around the central atom and the molecular geometry of IBr2-

a)

0 lone pairs, linear

b)

1 lone pair, bent

c)

2 lone pairs, bent

d)

3 lone pairs, bent

e)

3 lone pairs, linear

5.

the geometry of the SF molecule is

a)

tetrahedral

b)

trigonal pyramidal

c)

trigonal planar

d)

square planar

e)

distorted tetrahedron (seesaw)

6.

the geometry of the CIF3 molecule is

a)

tetahedral

b)

t-shaped

c)

trigonal planar

d)

square planar

e)

distorted tetrahedron (seesaw)

7.

According to the VSEPR theory which one of the following species has a tetrahedral geometry?

a)

IF4+

b)

IF4-

c)

PCI4+

d)

PCI4-

e)

SeF4

8.

According to the VSEPR theory which one of the following molecules is trigonal bipyramidal ?

a)

SF4

b)

XeF4

c)

NF3

d)

SF6

e)

PF5

9.

A molecule with 3 single bonds and 0 lone pairs of electrons is predicted to have which type of molecular geometry?

a)

Trigonal planar

b)

trigonal pyramidal

c)

trigonal bipyramidal

d)

bent

e)

linear

10.

A molecule with 2 single bonds and 2 lone pairs of electrons is predicted to have which type of molecular geometry?

a)

Trigonal planar

b)

trigonal pyramidal

c)

trigonal bipyramidal

d)

bent

e)

linear

11.

which of the following molecules is nonpolar?

a)

NH3

b)

OF2

c)

CH3Cl

d)

H2O

e)

BeCl2

12.

what is the bond order of Cl2+?

a)

0

b)

0.5

c)

1

d)

1.5

e)

2

13.

based on MO diagram of B2

a)

has a bond order of one and is diamagnetic

b)

has a bond order of one and is paramagnetic

c)

has a bond order of two and is diamagnetic

d)

has a bond order of two and is paramagnetic

14.

According to the molecular orbital theory, what is the bond order in the O2+ ion?

a)

1

b)

1.5

c)

2

d)

2.5

e)

3

15.

A molecule with the formula $AX_4E$ uses _____ to form its bonds.

a)

sp^2 hybrid orbitals

b)

sp^3 hybrid orbitals

c)

sp^3d hybrid orbitals

d)

sp^3d^2

16.

which of the following correctly lists species in order of increasing bond length?

a)

$C_2-<C_2<C_2+$

b)

$C_2<C_2+<C_2-$

c)

$C_2-<C_2+<C_2$

d)

$C_2+<C_2<C_2-$

17.

which of the following statements relating to molecular orbital (MO) theory is incorrect?

a)

Combination of two atomic orbitals produces one bonding and one antibonding MO

b)

A bonding MO is lower in energy than the two atomic orbitals from which it is formed

c)

combination of two 2p orbitals may result in either $\sigma$ or $\pi$ MOs

d)

A species with a bond order of zero will not be stable

e)

in a stable molecule having an even number of electrons, all electrons must be paired

18.

This is a ____ orbital

a)

s

b)

px

c)

py

d)

pz

19.

this is a ___ orbital

a)

s

b)

px

c)

py

d)

pz

20.

this is a ___ orbital

a)

s

b)

px

c)

py

d)

pz

21.

Which of the following species has the largest dipole moment (most polar)?

a)

H2

b)

H2O

c)

H2S

d)

H2Se

e)

CH4

22.

Which of the following is an ionic compound?

a)

$Cl_2$

b)

$Br_2$

c)

$H_2$

d)

NaCl

Chem exam 2

Total questions: 22

Worksheet time: 11mins

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