Semester 1 Final Exam Review Problems
Chapter 1: Matter and Measurement
Classifying Matter; Elements and Atoms; Compounds and Molecules; Physical and
Chemical Properties; Physical and Chemical Changes; Units of Measurement; Precision Accuracy
and Experimental Error.
When 10.0g of marble chips (calcium carbonate) is treated with 50.0mL of hydrochloric acid
(density = 1.096g/mL), the marble dissolves, giving a solution and releasing carbon dioxide gas.
The solution weighs 60.4g.
How many liters of carbon dioxide gas are released if the density of
the gas is 1.798g/L?
Some bottles of colorless liquids were being labeled when the technicians accidentally mixed
them up and lost track of their contents.
A 15.0mL sample withdrawn from one bottle weighed
The technicians knew that the liquid was either acetone, benzene, chloroform, or carbon
tetrachloride (which have densities of 0.792g/cm
What was the identity of the liquid?
Chapter 2: Atoms and Elements
Protons, Electrons, and Neutrons: Development of Atomic Structure; Atomic Number
and Atomic Mass; Isotopes; Atomic Weight; Atoms and the Mole; The Periodic Table
Natural carbon, which has an atomic mass of 12.011amu, consists of carbon-12 and carbon-
Given that the mass of carbon-13 is 13.00335amu, what would be the average
atomic mass (in amu) of a carbon sample
prepared by mixing equal numbers of carbon atoms
from a sample of natural carbon and a sample of pure carbon-13?
A monoatomic ion has a charge of 2+.
The nucleus of the ion has a mass number of 62.
The number of neutrons in the nucleus is 1.21 times that of the number of protons.
electrons are in the ion?
What is the name of the element?
Chapter 3: Molecules, Ions, and Their Compounds
Molecules, Compounds and Formulas; Molecular Models; Ionic Compounds: Formulas,
Names and Properties; Molecular Compounds: Formulas, Names and Properties; Formulas,
Compounds and the Mole; Describing Compound Formulas (Percent Composition, Empirical vs.
Molecular Formula, etc.); Hydrated Compounds
A sample of metallic element X, weighing 3.177g combines with 0.6015L of O
normal pressure and 20.0
C) to form the metal oxide with the formula XO.
If the density of O
gas under these conditions is 1.330g/L, what is the mass of the oxygen?
The atomic mass of
oxygen is 15.9994amu.
What is the atomic mass of X?
What is the identity of X?