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100

Which of the following elements is a halogen?
A) Bromine (Br)
B) Sodium (Na)
C) Carbon (C)
D) Magnesium (Mg)
E) Phosphorus (P)

Bromine (Br)

100

Provide the name or formula for the following:

- aluminum sulfate

- CuCl2

- sulfur hexafluoride

- Cl2O7

Al2(SO4)2

copper (II) chloride

SF6

dichlorine heptoxide

100

Which compound below becomes a strong electrolyte when dissolved in water?

A) CCl4
B) NaCl
C)C6H12O6
D) CH3OH
E) H2

B) NaCl

100

Name the following acids and bases:

  1. HCl
  2. H2SO4
  3. NaOH
  4. NH3


1. hydrochloric acid

2. sulfuric acid

3. sodium hydroxide

4. ammonia

200

If the average energy value of fat is 3.80×104 J/g, how many calories of energy are produced from 25.0 grams of fat?

1 calorie (cal) = 4.184 J

2.27×105 cal

200

The mass of a neutron is 1.67×10−27 kg. What is the mass of the neutron in milligrams (mg)?

1.67×10−21mg

200

A gas has a volume of 10.0 L and is at a temperature of 300 K. If the temperature of the gas is increased to 600 K, what is the new volume of the gas, assuming pressure and the amount of gas stay constant?

20.0 L

200

In each of the following equations, identify the Brønsted–Lowry acid and base in the reactants:

A. HCl(aq)+H2O(l)→H3O+(aq)+Cl−(aq)
B. HF(aq)+H2O(l)→H3O+(aq)+F−(aq)
C. NH3(aq)+H2O(l)→NH4+(aq)+OH−(aq)

  • A.

    • Acid: HCl
    • Base: H2O

  • B.

    • Acid: HF
    • Base: H2O

  • C.

    • Acid: NH4+
    • Base: OH−
300

The ground-state electron configuration of the element ________ is [Ar]4s23d5.
A) Mn
B) Cr
C) Fe
D) Co
E) Ti

Cr (Chromium)

300

Calculate the number of sulfur atoms in a 150 g sample of SO2. 

1.41×1024 sulfur atoms

300

How much NaCl is in 500 g of a 12.5% (m/m) NaCl solution?

62.5 g

300

For the reaction of acetic acid and water, which is the stronger acid in the equilibrium?

CH3COOH(aq)+H2O(l)⇌CH3COO−(aq)+H3O+(aq)

acetic acid

400

Arrange the following elements in order of increasing ionization energy:
Na, Al, S, Cl

Na < Al < S < Cl

400

Rank the following compounds by increasing boiling point: NH3, CH2Cl2, H2, H2O

H2O, NH3, CH2Cl2, H2

400

Based on the solubility guidelines, which of the following cations would form a precipitate in water with carbonate (CO32−) anion but not with sulfate (SO42−) anion?

A) Ca2+
B) Ba2+
C) Mg2+
D) Fe3+

C) Mg2+

400

What is the equilibrium concentration of HClO if the equilibrium concentrations of ClO− and H3O+ are each found to be 3.1×10−3 M?

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)

Ka=2.8×10−8

345 M

500

A hypothetical element Y has two naturally occurring isotopes. The percent (%) abundance and atomic mass of each isotope are given below:

Isotope 1 - 25.00% abundance, 10.00 amu

Isotope 2 - 75.00% abundance, 11.00 amu

What is the average atomic mass of element Y?

10.75 amu

500

Draw the lewis structure for CH2O and the dipole arrows. What is the polarity of the compound as a whole? How many bonding and non-bonding electrons are present?

polar compound

8 bonding electrons

4 non-bonding electrons

500

According to the reaction given below, how many grams of solid Cu(OH)2 are formed when 150 mL of 3.50 M aqueous NaOH reacts with excess aqueous CuSO4? (Note: Molar Mass of Cu(OH)2 is 97.57 g/mol)

CuSO4(aq)+2NaOH(aq)→Cu(OH)2(s)+Na2SO4(aq)

25.6 grams of Cu(OH)2

500

Write a balanced chemical equation for the following reactions of acids:

  1. HCl(aq)+Cu(OH)2(s)
  2. HNO3(aq)+Na2CO3(s)

1. HCl(aq)+Cu(OH)2(s)→CuCl2(aq)+2H2O(l)

2.HNO3(aq)+Na2CO3(s)→NaNO3(aq)+CO2(g)+H2O(l)