1. He could tell from the elements surrounding
#24 Why did Mendeleev leave spaces in
his periodic table?
He could tell from the elements surrounding
the “holes” in his table that they must exist.

2. the properties and existence of unknown elements made
#25 What effect did the discovery of gallium have
on the acceptance of Mendeleev’s table?
His ability to predict
the properties and existence
of unknown elements made
his table much more believable

3. #26 What pattern is revealed when
the elements are arranged in a
periodic table in order of increasing
atomic number?
Many trends are revealed such as
electronegativity, atomic and ionic radii,

4. #27 Based on their locations in the
periodic table, would you expect
carbon and silicon to have similar
properties?
Yes, they
are in the
same group

5. #28 Identify each property below as
more characteristic of a metal or a
non-metal.
a. gas at room temp.
non-metal, think of
oxygen gas

6. #28 Identify each property below as
more characteristic of a metal or a
non-metal.
b. brittle
non-metal, think of
a piece of lead in
your pencil--Carbon

7. #28 Identify each property below as
more characteristic of a metal or a
non-metal.
c. malleable.
metal: think of
pounding a piece
of gold into leaf with a
mallet.

8. non-metal: think of how well
metal conducts electricity. ie.
a wire.
#28 Identify each property below as
more characteristic of a metal or a
non-metal.
d. poor conductor of electric current.

9. #28 Identify each property below as
more characteristic of a metal or a
non-metal.
e. shiny.
metal: think of a shiny
piece of silver or gold.

10. Metalloids have properties that are
similar to both metals and non-metals.
How a metalloid behaves depends on
the conditions.
#29 In general, how are metalloids
different from metals and nonmetals?

11. #30 Where are the alkali metals, the
alkaline earth metals, the halogens,
and the noble gases?

12. #31 Which of the following are symbols for representative elements: Na Mg Fe Ni Cl
YES
YES NO NO
YES

13. #32 Which noble gas does not
have eight electrons in its highest
occupied energy level?
Helium;
it only has two
all others
have 8 valence
electrons

14. #33 Which of these metals isn’t
a transition metal?
a. aluminum
b. silver
c. iron
d. zirconium
Transition metals are light blue in this
table

15. #34 Use figure 6.12 to write the
electron configuration of these
elements.
a. B b. As c. F d. Zn e. Al

16. #35 Write the electron configurations
of these elements:
a. the noble gas in
period 3
b. the metalloid in
c. the alkali metal in period 3
Ar: 1s22s22p63s23p6
Si: 1s22s22p63s23p2
Na: 1s22s22p63s1

17. #36 Which element in each pair
has atoms with a larger atomic
radius?
a. sodium,
lithium

18. #36 Which element in each pair
has atoms with a larger atomic
radius?
b. strontium
magnesium

19. #36 Which element in each pair
has atoms with a larger atomic
radius?
c. carbon
germanium

20. #36 Which element in each pair
has atoms with a larger atomic
radius?
d. selenium
oxygen

21. #37Explain the difference between the first and second ionization energy of an element.
First ionization energy
is the energy
required to remove
the FIRST electron
Second ionization
energy is the energy
required to remove the
SECOND electron. It
is always GREATER
THAN the first ion-
ization energy

22. #38 Which element in each pair has
a greater first ionization energy?
lithium
boron
Boron

23. #38 Which element in each pair has
a greater first ionization energy?
magnesium
strontium
Magnesium

24. #38 Which element in each pair has
a greater first ionization energy?
cesium
aluminum
Aluminum

25. #39 Arrange the following groups
of elements in order of increasing
ionization energy. Sr Mg Be

26. #39 Arrange the following groups
of elements in order of increasing
ionization energy. Cs Ba Bi

27. #39 Arrange the following groups
of elements in order of increasing
ionization energy. Na Al S

28. Atomic Radius as compared
to IONIC radius
Atoms in elemental form (same #
of electrons as protons)
Ions

30. 1 1 1 1 1