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Worksheets

Pre-SAT 3

Total questions: 45

Worksheet time: 1hrs 5mins

Name
Class
Date
1.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
2.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
3.

Valence electrons are

a)

neutral (no charge)

b)

found in the outer most energy level of the atom

c)

equal to the number of protons

4.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

5.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

6.

Select the 3 exceptions to octet rule.

a)

Expanded octet

b)

Even number electron

c)

Incomplete octet

d)

Odd number electron

7.

Which of the following is true about expanded octets? (Check all that apply.)

a)

Any element can have an expanded octet.

b)

Elements in row 3 until 7 on the periodic table can have expanded octets.

c)

An expanded octet is when an element has less than 8 electrons.

d)

An expanded octet is when an element has more than 8 electrons.

e)

An expanded octet is when an atom has an unpaired set of electrons in its outer shell.

8.

Draw the Lewis structure for BH3 on your own. Then compare your drawing to the answer choices, and select the correct drawing for BH3.

a)
b)
c)
d)
9.

Draw the Lewis structure for BeI2. Then compare your drawing to the answer choices, and select the correct answer choice.

a)
b)
c)
d)
10.

What is incorrect about the following Lewis structure for SO3?

a)

Oxygen is not fulfilling the octet rule.

b)

Sulfur is not fulfilling the octet rule.

c)

All 24 valence electrons are not being used.

d)

There are too many valence electrons being used.

11.

What is the formal charge on the oxygen atom at the top of this Lewis structure?

a)

0

b)

-1

c)

+1

d)

-3

12.

What is the formal charge on the phosphorus atom in this Lewis structure?

a)

0

b)

-1

c)

+1

d)

-3

13.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
14.

What shape is shown here?

a)

Octahedral

b)

Tetrahedral

c)

Trigonal bipyramidal

d)

Seesaw

15.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
16.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
17.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
18.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

19.

Which one of these structural formula is non polar molecule?

a)
b)
c)
d)
20.

What is the molecular geometry/shape of HCN?

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

21.

Which of these is the shape of CCl4?

a)
b)
c)
d)
e)
22.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms.

b)

The difference in the electronegativities of the two atoms.

c)

The charges of the atoms.

d)

None of the above.

23.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

24.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

25.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
26.

BH3 molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

27.

HF molecules can form...

(choose all possible intermolecular forces)

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

28.

CH4 molecules can form...

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

29.

CH3Cl molecules can form...

(choose all possible intermolecular forces)

a)

London dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen bonds

30.

Which type of intermolecular force is the strongest?

a)

Hydrogen bonding

b)

Dipole-Dipole

c)

London Dispersion

31.

which of following forces is the weakest intermolecular force?

a)

Ionic bond

b)

Hydrogen bond

c)

Covalent bond

d)

van der Waals forces

32.

Intermolecular forces for: CO2

a)

London Force

b)

Dipole dipole

c)

Hydrogen bonding

33.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
34.

The diagram shows metallic bonding.


Which labels are correct?

a)

X: atomic nucleus

Y: outer electron

b)

X: metal atom

Y: mobile electron

c)

X: metal cation

Y: mobile electron

d)

X: positive ion

Y: negative ion

35.

Why do metallic compounds conduct electricity as solids?

a)

core electrons are mobile, allowing electricity to flow through the metal

b)

valence electrons are mobile, allowing electricity to flow through the metal

c)

protons are mobile, allowing electricity to flow through the metal

d)

the metal cations are mobile, allowing electricity to flow through the metal

36.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
37.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
38.

At equilibrium, __________.

a)

all chemical reactions have ceased

b)

the rates of the forward and reverse reactions are equal

c)

the rate constants of the forward and reverse reactions are equal

d)

the limiting reagent has been consumed

39.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
40.

Which is the reactant and why?

a)

A, it's concentration is decreasing

b)

A, it's concentration is increasing

c)

B, it's concentration is decreasing

d)

B, it's concentration is increasing

41.

At what time on the graph will the reaction reach equilibrium?

a)

t1

b)

t2

c)

t3

d)

t4

42.

What is the equilibrium-constant expression for

CO2(g) + H2(g) ↔ CO(g) + H2O(l)

a)

K= [CO][H2O] / [CO2][H2]

b)

K= [CO2][H2] / [CO]

c)

K= [CO2][H2] / [CO][H2O]

d)

K= [CO] / [CO2][H2]

43.
What is [A] and [B]?
a)
Concentration of Reactants
b)
Concentration of Products
c)
Energy of Reactants
d)
Energy of Products
44.
What was the equation for this reaction? All the substances were gases.
a)
A + B ⇌ 2C
b)
2A + B ⇌ 2C
c)
2C ⇌ 2A + B
d)
A2 + B ⇌ C2
45.
N2O4(g) ⇌ 2NO2(g)
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2 / [N2O4]
b)
Kc = [N2O4] /[ NO2]2
c)
Kc = [N2O4]2 / [NO2]
d)
Kc = [N2O4] x [NO2]2

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