Transcript period 2 - New York Science Teacher

Kenneth E. Schnobrich
Atomic Mass
6.941
Atomic
Number
+1
Li
3
1s22s1 or 2-1
Electron Configuration
Oxidation
State
GROUPS
VERTICAL COLUMNS -
H
• Alkali Metals
1
• Alkaline Earth Metals
2
• Transition Elements
3-12
• Chalcogens
16
• Halogens
17
• Inert (Noble) Gases
18
Li
Na
K
Rb
PERIODS
1s22s1
1s22s2
1s22s22p1
HORIZONTAL ROWS the Period Number
indicates the Principal
Energy Level that is filling
as we move from left to
right.
1s22s22p2
1s22s22p3
1s22s22p4
1s22s22p5
1s22s22p6
Li
Be
B
C
N
O
F
Ne
PERIODS
2-1
2-2
2-3
HORIZONTAL ROWS the Period Number
indicates the Principal
Energy Level that is filling
as we move from left to
right.
2-4
2-5
2-6
2-7
2-8
Li
Be
B
C
N
O
F
Ne
METALS
METALLOIDS
NONMETALS
INERT GASES
Table S*
DECREASES
*NYS Reference Tables for Chemistry
COVALENT RADII - PERIOD 2
1.4
1.2
1
0.8
Cov.Radii(A) Per.2
0.6
0.4
0.2
0
3
4
5
6
7
8
9
10
INCREASES
COVALENT RADII - GROUP IA
2.5
2
1.5
Cov.Radius(A)IA
1
0.5
0
1
3
11
19
37
55
Covalent Radius - effective distance
from the center of the nucleus to the
outer valence shell in a covalent or
coordinate covalent bond.
Van der Waals Radius - half the closest
distance between two nonbonded atoms.
Metals
+
Loss of electrons
Nonmetals
Gain of electrons
-
IONIZATION ENERGY
ELECTRONEGATIVITY
Definitions
Ionization Energy – the amount of energy (usually in
kilojoules) needed to remove the most loosely bound
electron from a gaseous atom of an element.
Electronegativity – the attractive force that an atom has
for an electron(s) during the formation of a chemical
bond. (no units are assigned)
“PROPERTIES OF SELECTED ELEMENTS”
Table S
496
Na
0.9
First Ionization
Energy (kJ/mol)
Electronegativity
INCREASES
General Trend Across a Period
600
500
400
300
I.E.(kcal) 2
200
100
0
3
4
5
6
7
8
9
10
DECREASES
General Trend Down a Group
350
300
250
200
I.E.(kcal) IA
150
100
50
0
1
3
11 19 37 55
General Trend Down a Group
350
300
250
200
I.E.(kcal) IA
150
100
50
0
1
3
11 19 37 55
Table S*
DECREASES
*NYS Reference Tables for Chemistry
Electronegativities of Group IA
2.5
2
1.5
IA
Electronegativity
1
0.5
0
1
3
11
19
37
55
Electronegativity Across a Period
INCREASES
Electronegativities for Period 2
4.5
4
3.5
3
Period 2
Electronegativities
2.5
2
1.5
1
0.5
0
3
4
5
6
7
8
9 10
REACTIVITY
REACTIVITY
INCREASES
INCREASES
 Multiple Oxidation States
 Form Colored Compounds
 Incomplete Inner “d” Sublevels
The Most active metals are in
Group  1 (IA)
 15 (VA)
 13 (IIIA)
 17 (VIIA)
The elements known as Alkali
metals are found in Group
 1 (IA)
 2 (IIA)
 13 (IIIA)
 17 (VIIA)
What is the total number of
electrons found in the valence
shell of an Alkaline Earth
element in the ground state
1
2
3
4
As the elements in Group IIA
are considered from top to
bottom, the # of electrons in the
2s subshell
 increases
 decreases
 remains the same
Which group contains atoms
that form +1 ions having an
inert gas configuration?
 1 (IA)
 11 (IB)
 17 (VIIA)
 7 (VIIB)
Which Group 17(VIIA)
elements listed below has the
greatest nuclear charge?
F
 Cl
 Br
I
Which element is most likely to
form a compound with Kr?
 Fluorine
 Chlorine
 Bromine
 Iodine
Which group on the Periodic
Table contains solid, liquid,
and gaseous elements at room
temperature?
 18 (O)
 2 (IIA)
 16 (VIA)
 17 (VIIA)
Which represents the correct
order of activity for the Group
VIIA(17) elements?
 Br > I > F > Cl
 F > Cl > Br > I
 I > Br > Cl > F
 F > Br > Cl > I
If the elements are considered
from top to bottom in Group
16(VIA), the number of
electrons in the outermost shell
will?
 decrease
 increase
 remain the same
Which Group contains and
element that is a liquid at room
temperature?
 18 (O)
 2 (IIA)
 11 (IB)
 12 (IIB)
Which element has the greatest
tendency to gain electrons?
 Te
 Se
S
O
USE CHART S
When atoms of the elements in
Group 18 (0) are compared in
order from top to bottom, the
attractions between atoms?
 increases and the boiling point decreases
 decreases and the boiling point increases
 increases and the boiling point increases
 decreases and the boiling point
decreases
In the ground state, an atom of
which element in Period 3 has
the most loosely bound
electron?
 Si
 Na
S
 Ar
USE CHART S
Which Period contains
elements that are all gases at
STP?
1
2
3
4
Considered in succession, the
elements in Period 2 of the
Periodic Table show a decrease
in atomic radius with
increasing atomic charge
increases?
 nuclear charge increases
 # of PEL increases
 number of neutrons decreases
 # of protons increases
Which represents the electron
configuration of a metalloid in
the ground state?
 2-3
 2-5
 2-8-5
 2-8-6
In a given Period of the
Periodic Table, the element
with the lowest first ionization
energy is always?
 an Alkaline Earth Metal
 an Alkali Metal
USE CHART S
 a Halogen
 an Inert Gas
As one goes from Li to F in
Period 2 of the Periodic Table,
the atomic radius of the
elements?
 decreases
 increases
 remains the same
USE CHART S
An element in which electrons
from more than one energy
level may be involved in bond
formation?
 potassium
 calcium
 copper
 zinc
Which element can form more
than one binary compound
with chlorine?
 potassium
 calcium
 iron
 zinc
A pure compound is blue in
color. It is most likely a
compound of?
 sodium
 lithium
 calcium
 copper
Which is the electron
configuration of a transition
element in the ground state?
 2-8-8
 2-8-8-2
 2-8-18-2
 2-8-18-8
Ar
Ca
Zn
Kr