Honors Chemistry - Chapter 6 Review Answers
Name: ___________________________
Section 6.1: Organizing the Elements
1. Group 1 on the periodic table is called Alkali Metals
2. Group 2 on the periodic table is called Alkaline Earth Metals
3. Elements in groups 3-12 are called Transition Metals
4. Group 17 on the periodic table is called Halogens
5. Group 18 on the periodic table is called Noble Gases
6. Each period on the periodic table corresponds to a principal energy level
7.
The 2 series that make up the inner transition metals are Lanthanides and Actinides
8. Complete the following chart:
Element
Symbol Group # Period #
Group Name
Metal, Metalloid, Nonmetal
Zirconium
Zr
4
5
Transition Metals
Metal
Radium
Ra
2
7
Alkaline Earth Metals
Metal
Bismuth
Bi
15
6
Nitrogen Group
Metal
Gallium
Ga
13
4
Boron Group
Metal
9. What are triads? Sets of 3 elements with similar properties Whose idea were they? Dobereiner
10. The modern periodic table is arranged by increasing atomic number. Whose idea was this? Moseley
11. Mendeleev developed the first periodic table, which was arrange by increasing atomic mass
12. Determine which of the following pairs will have similar properties (Yes or no):
a. Ca and Be? Yes – same group (Group 2 – Alkaline Earth Metals)
b. Sr and Y? No – not the same group
c. C and Ge? Yes – same group (Group 14 – Carbon Group)
Section 6.3: Periodic Trends
1. As you go across a period, the atomic radius (size) decreases because the attraction between protons
and electrons increases, which makes the atom smaller (opposite of tug of war)
2. As you go down a group, the atomic radius (size) increases because the number of principal energy
levels increases
3. Circle the atom with the largest atomic radius and put a square around the atom with the smallest radius:
a. Li
Ne
F
B
b. N
Bi
S
P
c. Na
Sr
Al
Cl
4. Ionization energy is the energy required to remove an electron.
Honors Chemistry - Chapter 6 Review Answers
Name: ___________________________
5. As you go across a period, ionization energy increases because the atom becomes more stable with
more valence electrons, thus the atom does not want to lose any electrons (it would take a lot of
energy to remove one)
6. As you go down a group, ionization energy decreases because the valence electrons are farther away
from the nucleus and more shielded (see question 8 for more detail).
7. Why do you think second ionization energy is higher than first ionization energy? Second ionization
energy is the energy required to remove a second electron. It is more difficult to remove a second
electron (because the attraction between protons and electrons increases).
8. Explain how the shielding effect determines the trend in ionization energy: Ionization energy decreases
as you go down a group because the atom increases in size, which means that there are more
shielding electrons between the valence electrons and the nucleus. The shielding electrons
“absorb” most of the attraction from the nucleus, so the valence electrons are not held as tightly.
It is easier to remove one of the valence electrons (lower ionization energy) because they are not
held as tightly by the nucleus.
9. Circle the atom with the highest ionization energy and put a square around the atom with the lowest
ionization energy:
a. Rb
Ru
Tc
b. Cu
Au
Ag
c. Cs
Fr
At
Sb
Rn
10. Electronegativity is the ability of an atom to attract an electron.
11. As you go across a period, electronegativity increases because the atoms have more valence electrons,
and want to attract electrons to obtain stability.
12. As you go down a group, electronegativity decreases because the valence electrons are farther away
from the nucleus (more shielded) and there is not a strong attraction from the nucleus to pull an
electron in.
13. Circle the atom with the highest electronegativity and put a square around the atom with the lowest
electronegativity:
a. B
Ga
Tl
In
b. Li
Ne
Be
C
c. Mg
Cd
As
Kr
14. Metals form ions called cations that have a positive charge (lose electrons). Nonmetals form ions called
anions that have a negative charge (gains electrons).
15. A negative ion is larger than its parent atom because it gained electrons.
16. A positive ion is smaller than its parent atom because it lost electrons.
Honors Chemistry - Chapter 6 Review Answers
Name: ___________________________
17. Circle the smallest atom/ion. Put a square around the largest atom/ion.
a. Cu
Cu+
Cu2+
b. N
N-
N3-
c. C4-
C2-
C
18. What is the most active metal? Francium (Fr)
19. What is the most active nonmetal? Fluorine (F)
C2+
C4+