DO NOW!

1
DO NOW! Suppose you have just discovered three
new elements. Element 1 is a solid at room
temperature, a fair conductor of heat and
electricity, and not ductile. Element 2 is a
solid at room temperature and shiny. Element 3
is a gas at room temperature and a poor conductor
of heat and electricity. Classify each element
as either a metal, non-metal, or metalloid.
A certain element belongs to the p-block. It
exhibits only moderate conductivity, is a solid
at room temperature, and is not malleable or
ductile. Further, it contains 4d electrons, but
not 5d electrons. It is also known not to have
chemical properties similar to those of nitrogen.
Identify the element and explain your reasoning.
2
40 Why is there a large increase in between the
first and second ionization energies of the
alkali metals?
Answer The alkali metals LOVE to lose
ONE electron to vacate the s-orbital that they
have half-filled. But to lose TWO electrons
would be too many. They want to achieve
the noble gas electron configuration.
noble gases
3
41 How does the ionic radius of a typical metal
compare with its atomic radius?
atomic radius
ionic radius
For Metals, the ionic radius is much
smaller because metals tend to LOSE electrons
from their outermost energy level.
4
42 Which particle has the larger radius in each
atom/ion pair?
a. Na, Na
Na
5
42 Which particle has the larger radius in each
atom/ion pair?
b. S, S-2
S-2
6
42 Which particle has the larger radius in each
atom/ion pair?
c. I, I-1
I-1
7
42 Which particle has the larger radius in each
atom/ion pair?
d. Al, Al3
Al
8
43. Which element in each pair has a higher
electronegativity value?
Cl and F
F
9
43. Which element in each pair has a higher
electronegativity value?
C and N
N
10
43. Which element in each pair has a higher
electronegativity value?
Mg and Ne
Neon has Zero electronegativity
Mg
11
43. Which element in each pair has a higher
electronegativity value?
As and Ca
As
12
44 Why are noble gases not included in table 6.2?
Because they have NO electronegativity they
cannot pull electrons in.
13
45 When the elements in each pair are chemically
combined which element in each pair has a greater
attraction for electrons?
The one with the highest electronegativity
Ca or O
O
14
45 When the elements in each pair are chemically
combined which element in each pair has a greater
attraction for electrons?
The one with the highest electronegativity
O or F
F
15
45 When the elements in each pair are chemically
combined which element in each pair has a greater
attraction for electrons?
The one with the highest electronegativity
H or O
O
16
45 When the elements in each pair are chemically
combined which element in each pair has a greater
attraction for electrons?
The one with the highest electronegativity
K or S
S
17
46 For which of these properties does lithium
have a larger value than potassium? a. first
ionization energy?
Lithium does
18
46 For which of these properties does lithium
have a larger value than potassium? b.
atomic radius?
Potassium does
19
46 For which of these properties does lithium
have a larger value than potassium? c.
electronegativity?
Lithium does
20
46 For which of these properties does lithium
have a larger value than potassium? d. ionic
radius?
potassium does
21

• The bar graph shows how many elements were
  discovered
• before 1750 and in each 50 year period between
  1750 and 2000
• In which 50 year period were the most elements
  discovered?
• b. How did Mendeleevs work contribute to the
  discovery of
• elements?
• c. What percentage of the elements were
  discovered by 1900?

1801 - 1850
Mendeleev's table predicted undiscovered elements.
75
22

• Write the symbol of the element or elements that
  fit each
• description
• a. a nonmetal in group 4A

4A
carbon
23

• Write the symbol of the element or elements that
  fit each
• description
• b. the inner transition metal with the lowest
  atomic number.

Lanthanium
24

• Write the symbol of the element or elements that
  fit each
• description
• c. all of the nonmetals for which the atomic
  number is a multiple of five.

25

• Write the symbol of the element or elements that
  fit each
• description
• d. a metal in group 5A

Bi
26
49 In which pair of elements are the chemical
properties of the elements most similar? Explain
your reasoning.
a. sodium and chlorine b.
nitrogen and phosphorus c. boron and oxygen
same group
27
50 Explain why fluorine has a smaller atomic
radius than both oxygen and chlorine.
Flourine is smaller than oxygen because it has
more protons pulling the electrons in tighter. It
is smaller than chlorine because it has 8
fewer electrons.
28
51 Would you expect metals or nonmetals in the
same period to have higher ionization energies?
Give a reason for your answer.
NON_METALS because the non-metals want to
retain electrons and even get more electrons not
lose them.
29
52 In each pair, which ion is larger?
Ca2 Mg2
Ca
30
52 In each pair, which ion is larger?
Cl-1 P-3
P-3
31
52 In each pair, which ion is larger?
The answer to this is not in the book!
Cu1 Cu2
Cu1
32
53 List the symbols for all the elements with
electron config. that ends as follows. Each n
represents an energy level.
a. ns1
33
53 List the symbols for all the elements with
electron config. that ends as follows. Each n
represents an energy level.
b. ns2np4
34
53 List the symbols for all the elements with
electron config. that ends as follows. Each n
represents an energy level.
c. ns2nd10
Not correctly written!
d orbitals are always lower than s or p orbitals!
35
54 Explain why there should be a connection
between an elements electron configuration and
its location on the periodic table.
An elements electron configuration
determines its location (group) in the periodic
table. It tells us how many valence electrons (s
and p sublevel).
36
55 Which equation represents the first
ionization of an alkali metal atom?
a. Cl NO, chlorine is not an alkali metal (it
is a halogen)
b. Ca NO, calcium is not an alkali metal (it
is an alkaline earth metal)
c. K K1 e- Yes this is an
alkali metal and it is giving off one electron.
d. H H1 e- NO, Hydrogen is
not considered an alkali metal even though it is
often listed in the same group
37
56 Use the graph in Fig 6.14 to estimate the
atomic radius of the indium atom.
Indium is Number 49 It appears to have a radius
of about 170 pm.
38
57 What trend is demonstrated by the following
series of equations? Li 520 kJ/mol
Li1 e- O 1314 kJ/mol
O1 e- F 1681 kJ/mol F1
e- Ne 2080 kJ/mol Ne1 e-
This information shows that ionization energy
increases as you go across a period from left to
right.
F
O
39
58 There is a large jump between the second and
third ionization energies of magnesium. There
is a large jump between the third and fourth
ionization energies of aluminum. Explain these
obser- vations.
Magnesium has TWO valence electrons (3s2) It
doesnt mind losing those two because then it has
10 electronsthe same as NEON, a noble gas. But
it doesnt want to lose a THIRD!!
40
58 There is a large jump between the second and
third ionization energies of magnesium. There
is a large jump between the third and fourth
ionization energies of aluminum. Explain these
obser- vations.
Aluminum has THREE valence electrons (3s23p1) It
doesnt mind losing those three because then it
has 10 electronsthe same as NEON, a noble gas.
But it doesnt want to lose a FOURTH!!
41
59 The bar graph shows the relationship between
atomic and ionic radii for Group 1A elements.
a. Describe and explain the trend in atomic
radius within the group.
The atomic radius increases from top to bottom
within the group.
42

• 59 The bar graph shows the relationship between
  atomic and ionic
• radii for Group 1A elements.
• Explain the difference between the size of the
  atoms and the sizes
• of the ions.

The since alkali metals all tend to lose one
electron, they become smaller because that outer
s orbital is now gone.