Name __________________________________
Date ______________________ Period ______
Periodic Trends Test Review
Decrease
1.
Draw the trend lines for atomic radius on the periodic
table to the right.
2. What is the definition of atomic radius?
Increase
Atomic Radii (Atomic Size)
Atomic radius is one half the distance between the nuclei
of two atoms (of the same element) that are bonded
together.
3. What happens to the size of atoms as you move down a group? Increases
Why? Down a group each element has an additional (and larger) energy level to hold its
electrons.
4. What happens to the size of an atom as you move left to right across a period? Decreases
Why? Across a period each successive element has an additional proton which increases the
positive charge in the nucleus. The positive charge attracts the negative electrons, and pulls
them toward the nucleus, making the atom smaller.
5. How are the numbers of valence electrons of the Group A elements related to the group
number? The group number tells you how many valence electrons elements in that group
have. For example, Group 1A elements each have 1 valence electron.
6. How is the energy level of an atom’s valence electrons related to the period it is in on the
periodic table? The period number tells you the energy level that an atom’s valence
electron(s) is/are located. For example, Sodium (Na) is in the third period. Its valence
electron is located in the 3rd energy level.
7. Put the following sets of elements in order of increasing atomic size (smallest to largest).
a.
Aluminum, Sodium, Chlorine
Cl, Al, Na
b. Rubidium, Lithium, Potassium
Li, K, Rb
c.
Xe, I, Sn
Tin, Iodine, Xenon
d. Bismuth, Phosphorous, Nitrogen
N, P, Bi
e.
Be, Ca, Ba
Beryllium, Barium, Calcium
8. Given any two elements within a group, is the element with the smaller or larger atomic
number likely to have a larger or smaller atomic radius than the other element?
The element with the larger atomic number will have the larger atomic radius.
9. Which has the largest radius: magnesium (Mg), silicon (Si), sulfur (S), or sodium (Na)? The
smallest?
Largest – Na
Smallest - S
10. Which has the largest radius: helium (He), xenon (Xe) or argon (Ar)? The smallest?
Largest – Xe
Smallest - He
Increase
Ionization Energy
Draw the trend lines for ionization energy on the periodic
table to the right.
2.
What is ionization energy?
Decrease
1.
The energy required to remove an electron from an atom.
3. Define an ion.
An ion is a charged particle.
4. Which group has the highest ionization energies? Explain why.
The noble gases have the highest ionization energy because they have 8 valence electrons
and therefore are very stable. They don’t want to lose electrons!
5. The octet rule explains why atoms sometimes form ions. What is the octet rule?
Atoms tend to gain, lose, or share electrons in order to acquire a full set of 8 valence
electrons like the noble gases.
6. An element forms a negative ion when ionized. On what side of the periodic table is the
element located?
The right side (it is a non-metal).
7. Which element in each pair has the larger ionization energy?
a.
Li, N
N
b. Kr, Ne
Ne
c.
Li
Cs, Li
Ionic Radius
1.
Decrease
Draw the trend lines for ionic radius on the periodic table
2. What is a cation? A positively charged particle.
3. Which elements typically form cations? Metals
Increase
to the right.
4. How are cations formed from these elements? Metal atoms lose electrons (which have a
negative charge) and thus become positively charged!
5. Are cations smaller or larger than the atoms from which they are formed? Smaller
6. What is an anion? A negatively charged particle.
7. Which elements typically form anions? Non-metals
8.
How are anions formed from these elements? Non-metal atoms gain electrons, which have a
negative charge, thus they acquire an overall negative charge.
9. Are anions smaller or larger than the atoms from which they are formed? Larger
10. Choose the element that will form an ion with the larger ionic radius.
a.
Boron, Oxygen
Oxygen (It is an anion and thus it is larger than the
cation that boron forms).
b. Fluorine, Iodine
Iodine
c.
Rubidium
Rubidium, Potassium
d. Magnesium, Phosphorous
Phosphorous (It is an anion and thus it is larger than
the cation that magnesium forms).
11. Imagine the following elements each formed ions. Put the elements in order of increasing
ionic radius.
a.
Ca, Be, Sr
Be, Ca, Sr
b. Cl, S, P
Cl, S, P
c.
Br, Se, As
As, Br, Se
d. Na, Sl, Mg
IGNORE THIS QUESTION – I made a typo! Oops! :0
e.
F, Cl, I
I, F, Cl
Increases
Electronegativity
Draw the trend lines for electronegativity on the periodic
table to the right.
2. Define electronegativity.
The ability of an atom to attract electrons toward itself
when it is bonded to another atom.
3. Which element is the most electronegative? Fluorine
Decreases
1.
4. Which element is the least electronegative? Francium
5. Explain how electronegativity of atoms in a bond has an effect on the electrons involved in
that bond.
The atom with the higher electronegativity will pull the electrons involved in
the bond toward itself.
6. Which element in each pair is more electronegative?
a.
K, As
As
b. N, Sb
N
c.
Be
Sr, Be
d. F, Fr
F
Chemical Families
1.
Color code the chemical families on the periodic table to the right according to the
following key:
a.
Alkali Metals – Red
b. Alkaline Earth Metals – Yellow
c.
1 2
1 2
3 4 5 6 7 8
13 14 15 16 17 18
Noble Gases – Purple
d. Transition Metals – Green
e.
Halogens – Orange
f.
Inner Transition Metals – Blue
2. Label groups 1A – 8A.
3. Now label these groups 1 – 18
4. What are group 1 elements called? How many valence electrons do group 1 elements have?
Alkali Metals. 1 valence electron.
5. What are group 2 elements called? How many valence electrons do group 2 elements have?
Alkaline Earth Metals. 2 valence electrons.
6. What are elements in the middle of the periodic table called?
Transition Metals
7. What are elements along the stair step called? Why?
Metalloids. They are called metalloids because they have properties of both metals and nonmetals.
8. What are elements in group 7A (17) called? How many valence electrons they have?
Halogens. 7 valence electrons.
9. What are group 8A (18) called? How many valence electrons do elements in group 8A have?
What is the exception?
Noble gases. Each noble gas has 8 valence electrons except Helium, which has 2.
10. Which family is the least reactive? Why?
Noble gases are the least reactive because they have a complete octet (8 valence
electrons), and thus are very stable.
11. Which metal family is the most reactive? Why?
Alkali metals are the most reactive metal family because they only have to lose 1 valence
electron in order to achieve a stable electron arrangement like the noble gases.
12. Which non-metal family is the most reactive? Why?
Halogens are the most reactive non-metal family because they only have to gain 1 valence
electron in order to achieve a stable electron arrangement like the noble gases.
13. Identify each of the following as an alkali metal, alkaline earth metal, transition metal, or
inner transition metal.
a.
Zirconium
Transition Metal
b. Gold
Transition Metal
c.
Inner transition metal
Uranium
d. Francium
Alkali metal
14. Identify each of the following as a metal, non-metal, or metalloid.
a.
Oxygen
non-metal
b. Barium
metal
c.
metalloid
Germanium
d. Iron
metal
e.
non-metal
Neon