Unit 3 Review
Chemistry
1. Label the periodic groups
#1
Alkali
#
2Alkaline
Metals
Earth
#7
Halogens
Metals
Transition Metals
# 8 Noble
Gases
2. Circle the most EN element and square the
least EN element
3. Highest IE red and lowest IE blue
Small atoms!
High IE and EN
Highest
EN
Lowest
IE
LARGE
atoms, low
IE and EN
5. Number the periods
6. Shade period 4 blue
groups
7. The rows are periods and the columns are _______________
1
2
3
4
5
6
7
increasing atomic #
8. The periodic table is organized by_______________
9. Use arrows to show the trend for
increasing atomic size/radius. Circle the
atom with the largest size/radius.
Metals (red – for review wksht)
 Nonmetals (blue for review wksht)
 Metalloids (green – for review
worksheet)

11) Have 1 valence electron
Alkali metals – group 1
____________________
12) Have 8 valence electrons
Noble Gases – group 18
____________________
13) Have 7 valence electrons
Halogens – group 17
____________________
14) Have 2 valence electrons
Alkaline Earth metals – Group 2
15) The least reactive elements
Noble Gases
____________________
16) The most reactive nonmetals (gases at
Halogens
room temperature)___________________
17) The most reactive metals
Alkali metals
____________________
18) Reacts explosively with oxygen and
Alkali
Metals
water
____________________
19) Used to make coins and jewelry.
Transition Metals
20) Energy required to remove an electron
Ionization Energy
from an atom____________________
21) The ability of atom to attract electrons.
Electronegativity
22) List 3 other elements that will have
similar chemical properties to Nitrogen
and explain why.
Most like: Phosphorus (P)
2nd most like: Arsenic (As)
3rd most like: Antimony (Sb)
Same group –gives them same # of valence electrons and
ion charge, therefore similar reactivity!
Circle the element in the pair has the larger
ionization energy. Explain why.
a. Li, N
b. Kr, Ne
c. Cs, Li
Closer to Fluorine!
Explain the octet rule.
Atoms will lose, gain, or share electrons to
have 8 valence electrons in their outer
energy level.
Circle the element in the pair is more
electronegative. Explain Why?
a. K, As b. N, Sb
c. Sr, Be
Smaller atoms – less shielding – nucleus charge is
stronger and can attract the electron more easily.
Periodic law states that elements show a
a. repetition of their physical properties
when arranged by increasing atomic radius.
b. repetition of their chemical properties
when arranged by increasing atomic radius.
c. periodic repetition of their properties when
arranged by increasing atomic number.
d. periodic repetition of their properties
when arranged by increasing atomic mass.
Elements in the same group of the periodic table
have the same:
a. number of valence electrons
b. physical properties
c. number of electrons
Which of the following is NOT true of an atom,
other than Helium, obeying the octet rule?
a. obtains a full set of 8 valence electrons
b. acquires the valence electrons of a noble gas
c. possess 8 electrons in total
d. has a s2p6 valence configuration
Moving down the periodic table, which two
atomic properties follow the same trend?
a. atomic radius, ionization energy
b. atomic radius, electronegativity
c. ionization energy, electronegativity
d. none of the above
Which will form a larger ionic radii than its’
parent atom?
a. cation (+ ion) b. anion (- ion)
Explain your choice!
Extra electrons cause repulsion and
cloud spreads out – ion gets bigger!
23) How many electrons does an atom of
8 total
Oxygen have? _____
6
How many valence electrons?________
10 total, 8
-2
How many electrons does 0 have? _____
valence
24) Fluorine has a higher ionization energy
than oxygen because fluorine has a larger
NUCLEAR/positive
____________ charge (why fluorine holds
on to its electrons so well)
2
1s
2
2s
6
2p
2
3s
6
3p
2
4s
25) Which element is this for?
Calcium
____________________26) In which period is this element found
2
4
in?______
In which group #? _______
27) How many electrons are in this
8
element’s 3rd energy level? _____
28) Re-write the electron configuration of
this element if it became an ion with a +2
charge 1s2 2s2 2p6 3s2 3p6
It loses the 2 electrons in 4s
Cloud Shaped
29) What is an orbital? A ____________
shaped region of an atom where an
Electron
____________
is most likely to be found.
30) How many orbitals (circles) are in each
3
1
sublevel? a. S = ___
b. P = ___
5
7
c. d = ___
d. F = ____
31) How many electrons can fit into 1
2 electrons
orbital? _____
32) Is the following electron sketch correct?
Explain
3s
3p
4s
3d
It is not correct, the 3d orbitals should have one in each
orbital and then it should double up!
33) Label the following blocks
34) Identify the blocks where these groups
are found –
p block
a. Halogens = ____
s
b. Alkaline Earth Metals = _____
block
s
c. Alkali Metals = ______
block
f
d. Rare Earth Metals = ______
block
p
e. The Noble Gases = _____
block
d
f. The Transition Metals = _______
block
35)
Identify
the
spectrum
A: Hydrogen &
Helium
B: Helium, Barium, Sodium
C: Barium, Calcium, Hydrogen, Helium
Photons and the Electromagnetic Spectrum
36) An electron that is closest to the nucleus
possible (at the lowest energy level
possible) is said to be in its ___________
_________________.
Ground State
37) When an electron jumps up to a higher
energy level and then falls back to its
Photon
ground state a ___________
is released.
Photons and the Electromagnetic Spectrum
38) The amount of energy released by an electron
jumping from the 4th energy level back to its
ground state at the 3rd energy level will always
release a photon with
a___________________________ (differentvariable/specific-quantized) amount of
energy.
39) The color spectra (types of colors produced) of
a star can be used to identify the types of
Elements
______________
present in the star.