Random
Atomic/Ionic
Radius
Radius
Ionization Energy
Coulombic Attrraction
Periodic Table
100
Which of the following elements have similar chemical properties?
A) Na, K, Ca
B) Mg, Ca, Ba
C) Ne, Ar, Kr, I
D) F, Cl, B
B) Mg, Ca, Ba
100
Atomic Radius ______ across a row and ______ down a group
Decreases; Increases
100
Ionization Energy ____ across a row and ____ down a group
Increases; Decreases
100
The force of attraction ___ across a row and ____ down a group
Increases; Decreases
100
____ is the most electronegative element
Fluorine
200
Choose the correct group or family that would have the highest first ionization energy
A) Halogens
B) Noble Gases
C) Alkali Metals
D) Alkaline Earth Metals
B) Noble Gases
200
The radius of cations generally ____ across a row.
Decrease
200
Which has the highest Ionization Energy:
A) Sn
B) Sb
C) As
D) Br
D) Br
200
Ca+2 or Ca has a greater force of attraction?
Ca+2
200
____ are the most reactive group of metals and ____ are the most reactive group of nonmetals.
Alkali Metals and Halogens
300
According to Coulomb's Law, as force increases, the charge _____; and the radius _______.
A) Decreases; Increases
B) Increases; Decreases
C) Decreases; Decreases
D) Increases; Increases
B) Increases; Decreases
300
Choose the ion with the largest radius:
Al+3 or N-3
N-3
300
Arrange the following in order of decreasing ionization energy:
S P N
N > S > P
300
Which of the following has the greatest force of attraction:
K+ Cl- Ar
K+
300
Explain why noble gases don't have electronegativity values.
Electronegativity is ability to attract electrons in a bond. Noble gases are stable with a full valence shell, therefore do not bond or attract electrons.
400
In comparing the effective nuclear charge of Cl- to F-, which one would be higher? When becoming an anion, would the atomic radius increase or decrease?
F-; increase
400
Based on the following Ionization Energies, identify the atom with the largest atomic radius.
A - 494
B - 577
C - 418
D - 1255
C - 418
400
Explain the difference in ionization between Mg and Al on the periodic table.
Mg - 738.1 kJ/mol
Al - 577.9 kJ/mol
Al requires less energy and is easier to remove since the p orbital is at a higher energy than the s orbital.
400
When comparing Coulombic attraction, identify the determining factor which has a greater effect on the force of attraction.
Distance to the outermost electron (Energy Level)
400
Identify the charges of the following elements:
K S Br Al
K+ S2- Br- Al3+
500
Justify why Oxygen has a lower first ionization energy than Nitrogen
Oxygens last electron is in a paired orbital creating electron-electron repulsion making it easier to remove.
500
Arrange the following in order of increasing radius:
Mg P-3 Al Ca+2 Cl-
Ca+2 < Mg < Al < Cl- < P-3
500
Identify the following element in period 2 given its ionization energies:
1st: 899 kJ/mol
2nd: 1757 kJ/mol
3rd: 14849 kJ/mol
Beryllium
500
Arrange the following in order of increasing Coulombic Attraction:
Mg+2 P-3 As Ca+2 F-1
P-3 < F-1 < As < Ca+2 Mg+2
500
Place the following in order of increasing reactivity:
Li Al K Ca Mg Na
Al < Mg < ca < Li < Na< K