Unit 4 Practice Exam
1.
2.
Period:
Name:
3.
What subatomic particles are found in the nucleus?
Give the name and charge for each of the three primary subatomic particles:
a.
b.
c.
How do you find the mass number of a certain isotope?
4.
What is the difference between mass number and atomic mass?
5.
What happens if somehow a proton were added to a nucleus of an atom?
6.
What happens if somehow a neutron were added to a nucleus of an atom?
7.
8.
9.
10.
11.
12.
Where is most of the mass of an atom located?
How much of the atom's volume is found in the nucleus?
What particle is mostly responsible for an atom's physical properties?
What particle is mostly responsible for an atom's chemical properties?
What "glues" the nucleus together?
What do you call atoms with the same number of protons, but different numbers of neutrons?
13. What are the most common isotopes of the following?
a. Carbon
c. Lead
b. Zinc
d. Chlorine
14.
Write the name of the Uranium isotope with 147 neutrons.
15.
Write the number of protons, Neutrons, and electrons, and isotope name for the following
neutral most common isotopes of the following:
a. Zr
b. Na
c. H
d. Mg
16.
A neutral atom has 19 electrons. What is the atom?
17.
An atom has 15 protons, 18 electrons, and 16 neutrons. What is the atom, what is its charge,
and what is its mass number?
18.
19.
20.
21.
A lithium atom with a total of 2 electrons is called a what?
What does the row number on the periodic table tell you?
What does the column numbers (on the A groups) of the period table tell you?
Draw Bohr diagrams of the following:
a. The most common
b. A +2 Cation of
c. A -2 Anion of
Oxygen atom.
Calcium.
Oxygen.
22.
For the following particles, write what the particle is, it’s charge, relative mass (1 being the
largest, so if one is ½ the size of the largest, you’d say ½ for that particle), & purpose (what
role does it play in the atom).
a. Proton-
b. Neutron-
c. Electron-
33.
34.
35.
36.
37.
38.
39.
40.
41.
Excluding the first energy level, the most stable electron configuration has how many
electrons in the valence shell?
Which ‘A’ group neutral elements fit in the following categories: highest Energy level (E),
number of valence electrons (V)
a. E1,V2
c. E3,V3
e. E4,V5
b. E3,V7
d. E5,V6
f. E5,V8
Find the highest energy level occupied (E) and number of valence electrons (V) in a neutral
atom of the following:
a. Gallium
c. Argon
e. Cesium
b. Tin
d. Phosphorus
f. Strontium
Why are the atoms in group 18 often called inert?
How many electrons will oxygen typically gain when it becomes ionic?
What type of ions do nonmetals form?
The group IIA elements will form what ion (include charge)?
The group VIA elements will form what type of ion when they are combined with a metal
(include charge)?
What are the most reactive elements (metal and nonmetal) in period 4 of the periodic table and
why?
42.
How do you know if an atom or ion has a stable electron configuration?
43.
44.
Which group of atoms have a naturally stable electron configuration?
What is electronegativity?
45.
How does electronegativity typically change on the periodic table?
a. Why is that?
46.
A metal and a nonmetal will typically have what type of bond?
47.
48.
49.
50.
51.
52.
53.
Two nonmetals will typically have what type of bond?
How can you predict if the bond between two elements will be ionic, polar covalent, or nonpolar covalent?
In ionic bonds, the sum of the charge of the cations and anions needs to be equal to
.
Nitrogen and Magnesium come together to form an ionic substance.
a. The element that forms the cations is
. The element that forms
the anions is
.
b. The symbol for the ionic form of nitrogen is:
and magnesium is:
c. The formula for the ionic compound will be:
If a compound is a molecule, you know that there is at least one
in the substance.
Which of the following is not a molecule?
a. SiO2
b. KCl
c. N2
d. C3H8
The formula for ionic compounds can be reduced (Mg2O2 = MgO), but covalently bonded
molecules cannot be reduced (C2H2 is the not the same as CH). Why is that?
54.
Ionic compounds typically have a
55.
Are ionic materials typically brittle or malleable?
56.
Ionic materials in solid form can generally be found in a(n)
structure, because
57.
Ionic materials typically conduct electricity when dissolved in water but do not in solid form.
Why is that?
58.
What information does a chemical formula give you?
59.
What is the difference between a single, double, and triple covalent bond?
60.
Given the formula of the following ionic compounds write the symbols for each ion.
a. MgBr2: ions –
b. KCl: ions –
c. Sr3P2: ions –
d. Na3N: ions –
Given the name of the following compounds write ionic symbols for each ion and the formula:
a. Sodium Nitride: ions –
formula –
b. Magnesium Phosphide: ions –
formula –
c. Aluminum Sulfide: ions –
formula –
d. Aluminum Bromide: ions –
formula –
61.
melting point because
Why?