Name
Date
Chapters 6 and 7 Review (with a little 4 & 5 thrown in)
Describe the location on the periodic table, and the characteristics (including valence electrons) of:
Alkali metals
Alkaline earth metals
Halogens
Noble gases
Transition metals
Electrons and the nucleus of an atom are involved in a tug of war; the nucleus tries to attract and hold the
valence electrons as closely as possible. The attraction between the nucleus and the valence electrons depends
on TWO main things: the positive charge in the nucleus (# of protons tugging) and the distance to the valence
electron, b/c of its E level and how many inner electrons are shielding it from the nucleus. These properties
explain the trends which provide the basis for periodic law. Review the periodic trends and be able to explain
how and why they change. An example for atomic size is shown below. You will need to know these for the test.
Atomic size decreases L to R. The # of protons increases L to R, but electrons are added in the
same energy level. So each electron added is being attracted to the nucleus by one added
proton. The nuclear pull on valence electrons increases, so the atoms get smaller L to R.
Atomic size increases as you go down a group because you are adding E levels, and electrons are
further away, so the nucleus can’t pull them in as tightly.
What is the element with the lowest electronegativity value?
a. Cesium
b. Helium
c. Calcium
d. Fluorine
Which of the following atoms forms ions with the smallest ionic radius?
a. Li
b. K
c. O
d. S
For Group 2A metals, which electron is the most difficult to remove?
a. the first
b. the second
c. the third
d. all electrons are equally difficult
Which of the following factors contributes to the decrease in ionization energy within a group in the periodic
table as the atomic number increases?
a. increase in atomic size
b. increase in the size of the nucleus
c. increase in number of protons
d. fewer electrons in the highest occupied E level
Which of the following elements has the smallest first ionization energy?
a. sodium
c. potassium
b. calcium
d. magnesium
Match each item with the correct statement below.
a. electronegativity
f. periodic law
b. ionization energy
g. cation
c. atomic radius
h. period
d. metal
i. group
e. transition metal
j. electrons
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1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
horizontal row in the periodic table
vertical column in the periodic table
repetition of properties occurs when elements are arranged by increasing atomic number
type of element that is a good conductor of heat and electric current
type of element characterized by the presence of electrons in the d orbital
one-half the distance between the nuclei of two atoms when the atoms are joined
type of ion formed by Group 2A elements
subatomic particles that are gained/lost to form positive or negative ions
ability of an atom to attract electrons when the atom is in a compound
energy required to remove an electron from an atom
Match each item with the correct statement below.
a. halide ion
e. valence electron
b. octet rule
f. coordination number
c. ionic bond
g. metallic bond
d. electron dot structure
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11.
12.
13.
14.
15.
16.
17.
Atom
1
H
an electron in the highest occupied energy level of an atom
atoms react so as to acquire the stable electron structure of a noble gas
a depiction of valence electrons around the symbol of an element
an anion of chlorine or other halogen
the force of attraction binding oppositely charged ions together
the attraction of valence electrons for metal ions
the number of ions of opposite charge surrounding each ion in a crystal
Period means
1 Energy level
Group means
1 valence electron
G/P diagram
®
Nucleus
Valence e –
1st E level
Forms ion(s)
H+
Na
Ca
N
S
The nucleus of an atom contains _______________ which are ______________ charged and ________________
which have _____ charge. The number of protons in the nucleus is the ___________________________ of the
atom, while the number of subatomic particles total in a nucleus is the _________________________________.
When two atoms have the same number of protons but different number of neutrons, they are still the same
_________________ but they are __________________ of each other. In a neutral atom, the number of
________________ is always equal to the number of _________________. When an atom gains electrons it
becomes more ________________ charged, and becomes an ________________ but if it loses electrons and its
charge becomes more __________________ then it is called a ___________________. The charge on an ion can
be calculated with the following equation: ionic charge = ______________ - _______________. Metals tend to
form ____________ while non-metals tend to form _______________. When these two kinds of ions are
attracted to each other they form an ionic bond, which forms a type of compound called a ______________.
Write out the electron configurations for the atoms/ions below.
K
K+
F-
F
What do the ions above have in common, and what rule is this?
Give an example of a different isotope with the common ion of each of the following atoms: (see example)
30
46
82
6
2
P
Sc
Br
Li
H  1H+
How many protons, neutrons, and electrons does each atom above have in your examples?
1 p+, 0 n, 0 e-
If you have the following isotopes, calculate the average atomic mass of element X. Show your work.
X = 4.34%,
X = 83.79%,
X = 9.50%,
X = 2.37%.
What are the rules for electrons filling orbitals?
Show the following electron configuration orbital diagrams correctly: Calcium, Zinc, and Sulfur.
When electrons are stimulated, they can jump to higher energy levels; each jump requires a specific amount of
energy called a _________________. When they fall back down they release a _____________, a small light
burst that we can see and measure.
The ____________________ (m) of electromagnetic radiation is the distance from the crest of one wave to the
next, while the rate at which they pass by is called the ___________________(sec-1). These two values are
_________________________ proportional to each other and when they are multiplied, they equal c, which is a
constant speed of light, equal to ____________________________.
If the wavelength of light is 2.5 x 10-9m, find the frequency and the part of the spectrum that it will be in.
If the frequency of a light wave is 5.34 x 1014 Hz, find the wavelength and where in the spectrum it will be.
What ions do the following elements likely form? Give your answers with symbols and charges.
Lithium
Aluminum
Oxygen
Iodine
Gold
Phosphorous
Barium
Manganese
Silver
Fluorine
What unit formula would best represent the following compounds, based on your previous answers.
Lithium oxide Aluminum fluoride
Silver iodide
Barium phosphide
Gold oxide
Compare and contrast ionic compounds (salts) and metals. Be thorough!