Download Chapter 1 Assignment Section 1.1 1. Why is air classified as matter

Chapter 1 Assignment
Section 1.1
1. Why is air classified as matter?
2. Explain the difference between physical chemistry and analytical chemistry.
Section 1.2
1. Give 3 reasons why a farmer would want to have some knowledge of chemistry.
2. Give 3 reasons why an Olympic athlete would want to have an understanding of chemistry.
Chapter 2 Assignment
Section 2.1
1. What is the relationship between the state of substance at room temperature and its boiling point?
2. Fingernail polish is a liquid at room temperature. The smell is due to a chemical called ethyl acetate.
Would the ethyl acetate in the gaseous state be classified as a vapor or a gas? Explain your answer.
Section 2.2
1. Classify the following mixtures at homo- or heterogeneous:
a) granite rock
b) salt water
c) chocolate chip ice cream d) a silver ring
2. What physical property is used to separate gases?
Section 2.3
1. Can compounds be separated into their components by physical processes?
2. Classify the following as element, compound or mixture:
a) table salt
b) salt water
c) sodium
Section 2.4
1. When powdered iron is left exposed to air, it will rust. Explain why the mass of the rust will be greater
than the mass of the iron.
2. A chemical change can be indicated by the production/appearance of an odor. Describe two situations
that you might be able to detect such a change in odor in a kitchen.
Chapter 4 Assignment
Section 4.1
1. What is an atom according to a) Democritis?
b) John Dalton?
Section 4.2.
1. Why are the relative charges and masses useful in talking about subatomic particles?
2. Why does it make sense that if an atom gains an electron it ends up with a negative charge?
Section 4.3
1. An atom has 11 protons 11electrons and 10 neutrons. What is its:
a) atomic number
2. For
b) mass number
c) name
d) complete symbol
b) number of electrons
c) name
d) number of neutrons
what is the:
a) number of protons
e) mass number
3. There are five naturally occurring isotopes of the element zinc. The relative abundance and mass of
each are as follows.
: 48.89%, 63.929 amu,
: 27.81%, 65.926 amu,
: 4.11%, 66.927 amu,
: 18.57%, 67.925
amu,
: 0.62%, 69.925 amu
Calculate the average atomic mass of zinc.
Chapter 5 Assignment
Section 5.1
1. How many orbitals are in the following sublevels:
a) 2s
b) 3p
c) 6d
d) 4p
Section 5.2
1. Write the full electron configurations for the following:
a) barium
b) lead
c) chromium
d) sulfur
2. Write the condensed electron for the following:
a) magnesium
b) bromine
c) arsenic
d) vanadium
Chapter 6 Assignment
Section 6.1
1. Give an example of :
a) an alkali metal
b) transition metal
c) lanthanide d) halogen
e) alkaline earth metal
f) metalloid
2. Name two elements that would have similar properties to potassium.
Section 6.2
1. What group of elements are characterized by an s2p3 configuration?
2. Identify the elements that have electron configurations that end as follows.
a. 2s22p4
b. 4s2
c. 4s23d10
3. Why would you expect Li and S to have different chemical and physical properties?
Section 6.3
1. Why is a magnesium atom smaller than a sodium atom and a calcium atom?
2. Would you expect a Cl― ion to be larger or smaller than Mg2+?
3. Which would have a larger first ionization energy?
a) Na or Li
b) Na or P?
4. Arrange oxygen, fluorine, and sulfur in order of increasing electronegativity.
Chapter 7 Assignment
Section 7.1
1. For each element below, state (i) the number of valence electrons in the atom,
(ii) the electron dot structure, and (iii) the chemical symbol(s) for the most
stable ion.
a. Ba
b. I
c. K
2. How many electrons are lost or gained in forming each of the following ions?
a. Mg2+
b. Br―
c. Ag+
d. Fe3+
Section 7.2
1. Use electron dot structures to predict the formula of the ionic compounds formed
when the following elements combine.
a. sodium and bromine
d. aluminum and oxygen
2. Which of these combinations of elements are most likely to react to form ionic
compounds?
a. sodium and magnesium c. potassium and iodine
b. barium and sulfur d. oxygen and argon
Section 7.3
1. What is an alloy?
2. Name the principal elements present in each of the following alloys.
a. brass
d. sterling silver
b. bronze
e. cast iron
c. stainless steel
f. spring steel
Chapter 8 Assignment
Section 8.1
1. Which of the following elements exist as diatomic molecules?
a) lithium
b) oxygen
c) sulfur
d) Iodine
2. What types of elements tend to combine to form molecular (covalent) compounds?
Section 8.2
1. Draw the electron dot structure of PI3
2. Draw the electron dot structure of HCP
Section 8.3
1. Draw the electron dot structure, line structure and state the molecular shape of the following
a) BI3
b) CH3F
Section 8.4
1. What type of bond—nonpolar covalent, polar covalent, or ionic—will form
between each pair of atoms?
a. Na and O b. O and O c. P and O
2. Predict the polarity of:
a) PI3
b) HCP
c) BI3 d) CH3F