Free Printable Honors Chemistry Unit 2 Test

1.

How long is the block, using sig figs?

a)

1.0 cm

b)

1.3 cm

c)

1.37 cm

d)

1.375 cm

2.

How many significant figures are in 34.50?

a)

3

b)

4

c)

5

d)

2

3.

How many sig figs are in 0.00780

a)

3

b)

2

c)

5

d)

4

4.

What is 3.45 + 7.12

a)

10.57

b)

10.6

c)

11

d)

10

5.

What is 13.45-1.2

a)

12.25

b)

12.3

c)

12.2

d)

12

6.

What is 9.21X 30

a)

276.3

b)

280

c)

3

d)

300

7.

Which answer is correct according to sigfigs: $\frac{23.2\ +\ 21.22}{36.2\ \times\ 30}=$

a)

.041

b)

.04

c)

.4

d)

.049

8.

Which of the following pairs of elements is most likely to form an ionic compound?

a)

magnesium and fluorine

b)

manganese and iron

c)

oxygen and chlorine

d)

sodium and aluminum

9.

What is the chemical formula of sodium nitride?

a)

NaN

b)

Na₂N

c)

Na₃N

d)

NaN₃

10.

What is the balanced chemical formula of iron (II) oxide?

a)

FeO

b)

FeO₂

c)

Fe₂O₂

d)

Fe₂O

11.

Select the correct formula for boron trichloride.

a)

B₂Cl

b)

B₃Cl

c)

BCl₃

d)

BCl₂

12.

MgCl2 + Na ---> NaCl + Mg

What type of reaction is shown by the equation?

a)

Combination/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

13.

___Fe + ___O₂ ---> ___Fe₂O₃

Which set of coefficients will correctly balance the equation?

a)

Already Balanced (no coefficients needed)

b)

2, 3, 4

c)

4, 3, 2

d)

3, 2, 2

14.

What is the charge of an atom that has lost one electron?

a)

-1

b)

-2

c)

+1

d)

+2

15.

Ionic bonds ...

a)

transfer (exchange) electrons to become stable

b)

Share electrons

c)

occur within a sea of electrons

16.

covalent bonds form between...

a)

metal and nonmetal

b)

nonmetal and nonmetal

c)

metal and metal

17.

Have a high melting point (1000°C-3000°C)

a)

ionic compounds

b)

covalent compounds

18.

Molten compound conducts electricity.

a)

ionic compound

b)

covalent compound

19.

H

a)

Diatomic

b)

Monatomic

20.

Br

a)

Diatomic

b)

Monatomic

21.

C

a)

Diatomic

b)

Monatomic

22.

Ca

a)

Diatomic

b)

Monatomic

23.

The charge of V in V₂O₅ is?

a)

2+

b)

3+

c)

4+

d)

5+

24.

The formula for iron_(III) oxide is

a)

FeO

b)

Fe₃O

c)

Fe₂O₃

d)

Fe₃O₂

25.

Name the following compound: NaNO₃

a)

Sodium Nitrogen Oxide

b)

Sodium nitrate

c)

Sodium nitrite

d)

Sodium nitride

26.

phosphorous acid

a)

H₃PO₄

b)

H₂PO₄

c)

H₃P

d)

H3PO3

27.

sulfuric acid

a)

HSO₃

b)

H₂SO₃

c)

H₂SO4

d)

H3SO4

28.

HF

a)

hydrofluoric acid

b)

Hypofluoric acid

c)

hydrogen fluorine acid

29.

Hydroiodic acid

a)

H2I2

b)

H1I1

c)

HI

30.

hydrochloric acid

a)

HCl

b)

_HClO

c)

H₃ClO₃

d)

HClO₃

31.

Potassium hydroxide

a)

KOH

b)

K2OH

c)

k(OH)2

32.

When the polyatomic ion in an acid ends in -ate, the root name of the polyatomic ion is followed by the ending -_____.

a)

ide

b)

ic

c)

ous

d)

ite

33.

Does HCl have hydrogen bonding?

a)

yes

b)

no

34.

All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces. Which of these has ONLY London forces?

a)

I₂

b)

NH₃

c)

OCl₂

d)

SH₂

35.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

36.

Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction

a)

dipole-dipole>covalent bond>hydrogen bond>London

b)

London>dipole-diple>hydrogen bond>covalent bond

c)

covalent bond>hydrogen bond>dipole-dipole>London

d)

hydrogen bond>dipole-dipole>London>covalent bond

37.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

38.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

39.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

40.

When you have C-H, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

41.

Translate the word equation below:

Nitrogen reacts with Hydrogen to form Ammonia (NH₃).

a)

$N\ \ \rightarrow\ H\ +\ NH_3$

b)

$N_2\ +\ H_2\ \rightarrow\ NH_3$

c)

$N\ +\ H\ \rightarrow\ NH_3$

d)

$N_2\ \rightarrow\ H_2\ +\ NH_3$

42.

Translate the word equation below.

Carbon Dioxide and Hydrogen react to form Methane (CH₄) and Water

a)

$CO_{2_{\ }}+\ H_2O\ \rightarrow\ CH_4\ +H_2\$

b)

$CO_2\ \rightarrow\ H_2\ +\ CH_4\ +\ H_2O$

c)

$CO_2\ \ +\ H_2\ +\ CH_4\ \ \rightarrow\ H_2O$

d)

$CO_2\ \ +\ H_2\ \rightarrow\ CH_4\ +\ H_2O$

43.

The following is what type of reaction:
PbCl₂ + AgNO₃ → Pb(NO₃)₂ + AgCl

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

44.

What type of chemical reaction is this?
Al(OH)₃ → Al₂O₃ + H₂O

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

45.

Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water.

a)

Decomposition

b)

Synthesis

c)

Combustion

d)

Single Replacement

46.

Predict the products for the following reactants.
Mg + I₂ -->

a)

MgI

b)

MgI₂

c)

Mg + I₂

d)

Mg₂I

47.

Predict the products for the following reactants.
C₆H₁₂ + O₂ -->

a)

CO + H₂

b)

CO₂ + O₂

c)

C₃H₆O

d)

CO₂ + H₂O

48.

Predict the products for the following reactants.

K₂CO₃ + BaCl₂ -->

a)

No Reaction

b)

KCl + BaCO₃

c)

K₂Cl + BaCO₃

d)

KCl₂ + BaCO₃

49.

Classify the reaction based on the reactants given:
$Na_2O\rightarrow$

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Single Replacement

e)

Double Replacement

Honors Chemistry Unit 2 Test

Total questions: 49

Worksheet time: 2hrs 47mins

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