Free Printable Honors Chemistry Semester 1 Review

1.

Which of the following is considered to be a physical property of matter?

a)

Reactivity

b)

pH

c)

Solubility

d)

Toxicity

2.

Which of the following is considered to be a chemical property of matter?

a)

Viscosity

b)

Reactivity

c)

Texture

d)

Density

3.

Which of the following would not be classified as a pure substance?

a)

Element

b)

Compound

c)

Solution

d)

Molecule

4.

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

5.

What is the correct Lewis Dot Structure for ammonia NH₃

a)

b)

c)

d)

6.

What is percent composition of the element hydrogen in the compound methane, CH₄?

a)

16.0%

b)

25.1%

c)

74.9%

d)

100%

7.

What is the percent composition, to two significant digits, for each element in sodium chloride (NaCl)?

a)

23% Na, 35% Cl

b)

39% Na, 61% Cl

c)

50% Na, 50% Cl

d)

61% Na, 39% Cl

8.

Describe one chemical change and one physical change in a burning candle.

a)

A chemical change is producing heat, and a physical change is emitting light in a burning candle.

b)

A chemical change is producing heat, and a physical change is melting wax in a burning candle.

c)

A chemical change is melting wax, and a physical change is producing heat in a burning candle.

d)

A chemical change is melting wax, and a physical change is emitting light in a burning candle.

9.

A list of the materials for a chemistry lab are provided.

1. A 3 cm long strip of magnesium

2. A 10 mL sample of hydrochloric acid

3. A stir rod with density greater than 1.5 g/mL

4. A beaker at room temperature

Which materials are listed with intensive properties?

a)

1 and 2

b)

2 and 4

c)

3 and 4

d)

1 and 3

10.

Substances with an indefinite shape and an indefinite volume are in which state of matter?

a)

Gaseous state

b)

Liquid state

c)

Solid state

d)

No state of matter fits this description

11.

What is an example of a pure substance?

a)

Air

b)

Alloy

c)

Salt water

d)

Oxygen

12.

The reactivity trends on the Periodic Table depends on valence electrons. What family on the Periodic Table is identified as the most reactive nonmetals?

a)

1

b)

12

c)

13

d)

17

13.

Alkali metals react very readily with halogens and form ionic compounds such as table salt (NaCI) and many others. Which of the following explanations most completely describes why these two families of elements reacts readily?

a)

Alkali metals are negative and halogens are positive, so they attract each other.

b)

The alkali metals have one valence electron, and the halogens are one short of an octet.

c)

Alkali metals and halogens can very easily share eight valence electrons between them.

d)

The halogens very easily donate valence electrons to the alkali metals so that all have eight.

14.

Using the Periodic Table, predict which elements will have similar chemical properties or reactivity.

a)

Cadmium, calcium, and carbon

b)

Magnesium, strontium, and barium

c)

Rubidium, yttrium, and zirconium

d)

Nitrogen, sulfur, and bromine

15.

Which statement best describes the name and location on the Periodic Table of the elements with the highest and lowest electronegativity, respectively?

a)

Fluorine, on the upper right, has the highest electronegativity, and Francium, on the lower left, has the lowest electronegativity.

b)

Helium, on the upper right, has the highest electronegativity, and Francium, on the lower left, has the lowest electronegativity.

c)

Neon, on the upper right, has the highest electronegativity, and Francium, on the lower left, has the lowest electronegativity.

d)

Hydrogen, on the upper left, has the highest electronegativity, and Radon, on the lower right, has the lowest electronegativity.

16.

Which of the following elements has the largest atomic radius?

a)

Calcium

b)

Sodium

c)

Potassium

d)

Magnesium

17.

Which of the following statements is most accurate regarding atoms?

a)

Most atoms cannot combine with other atoms.

b)

Chemical reactions divide atoms into smaller units.

c)

Atoms of the same element may have different mass numbers.

d)

Atoms only contain protons.

18.

Visible light has a higher frequency than radio waves on the electromagnetic spectrum. How does the wavelength of visible light compare to radio waves?

a)

Visible light has a longer wavelength than radio waves.

b)

Visible light has a shorter wavelength than radio waves.

c)

Visible light has the same wavelength as radio waves.

d)

Visible light does not have a wavelength while radio waves do have a wavelength.

19.

A sample of Element X is found to contain 72.15% of isotope type 1 (84.9118 amu) and 27.85% of isotope type 2 (86.9092 amu). Calculate the average atomic mass.

a)

85.13 amu

b)

85.47 amu

c)

86.21 amu

d)

86.49 amu

20.

The Lewis valence dot electron structures are used to illustrate the number of valence electrons of atoms of representative elements. Considering this, use the Periodic Table to predict the number of “dots” that should be drawn around Antimony (Sb) to represent its Lewis Dot Structure.

a)

2

b)

5

c)

6

d)

8

21.

What is the correct name for the following compound?

Li₂S

a)

Dilithium monosulfide

b)

Lithium disulfide

c)

Sulfuric lithate

d)

Lithium sulfide

22.

What is the correct name for the following compound?

H₂O

a)

Hydrogen oxide

b)

Hydrogen oxolate

c)

Dihydrogen monoxide

d)

Hydrogen dioxide

23.

What is the chemical formula for disulfur decafluoride?

a)

$S_{10}F_2$

b)

$S_3F_9$

c)

$S_2F_{10}$

d)

$S_2F_8$

24.

Which of the following is a possible compound formed from Ca²⁺ and NO₃^-1?

a)

$Ca_2NO_3$

b)

$Ca\left(NO_3\right)_2$

c)

$Ca_3NO_2$

d)

CaNO

25.

Choose the correct Lewis Dot diagram for MgO.

a)

b)

c)

d)

26.

Metals can conduct electricity and heat well due to —

a)

the ability of the electrons to move freely throughout the metal

b)

the attraction of the electrons to the energy of the kinesis

c)

the repulsion of protons from neutrons in the metal

d)

the energy which is inherent in the molecular mass of the metal

27.

Which of these statements describes the basic idea of the Valence Shell Electron Pair Repulsion (VSEPR) theory?

a)

There is always an octet of electrons around an atom in a molecule.

b)

Electrons are attracted to the nucleus of the central atom.

c)

Molecules repel one another due to intermolecular forces.

d)

Shared and unshared electron pairs repel each other as much as possible.

28.

What is the molar mass of sodium chloride, NaCl?

a)

53.02 g/mol

b)

58.44 g/mol

c)

102.8 g/mol

d)

112.5 g/mol

29.

How many Mg atoms are found in 1.00 mole of MgO?

a)

$3.01x10^{23}$

b)

$6.02x10^{23}$

c)

$1.20x10^{24}$

d)

$6.02x10^{25}$

30.

Calculate the number of molecules present in .20 moles of H₂O.

a)

$2.9x10^{25}\ molecules$

b)

$5.1x10^{22}\ molecules$

c)

$1.2x10^{23}\ molecules$

d)

$2.4x10^{23}\ molecules$

31.

Which of the following could represent a molecular formula for CH₂O?

a)

$C_2H_3O_2$

b)

$C_6H_{12}O_6$

c)

$C_4H_3O_4$

d)

$C_4H_2O_4$

32.

The reaction between solid aluminum and liquid bromine is exothermic. This reaction creates the product aluminum bromide. What equation includes the correct formulas and demonstrates conservation of mass?

a)

Al(s) + Br2(l) → AlBr3(s)

b)

Al(s) + Br(l) → AlBr(s)

c)

Al(s) + 3Br(l) → AlBr3(s)

d)

2Al(s) + 3Br2(l) → 2AlBr3(s)

33.

What are the coefficients that would correctly balance this equation?

____Zn + ____K₂CrO₄ → ____K + ____ZnCrO₄

a)

2, 1, 2, 1

b)

1, 2, 3, 1

c)

1, 2, 1, 2

d)

1, 1, 2, 1

34.

Methane is natural gas containing both carbon and hydrogen. What type of reaction occurs when methane reacts with oxygen gas to produce carbon dioxide, water, and energy?

a)

Synthesis

b)

Single-replacement

c)

Double-replacement

d)

Combustion

Honors Chemistry Semester 1 Review

Total questions: 34

Worksheet time: 20mins

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