Atomic Theory, Periodic Table And Chemical Bonding Worksheet
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1
2Review #2: Atomic Theory, Periodic Table and Chemical Bonding
1.
Define or explain the following terms:
Atom
Alpha-decay
Isoelectronic
Atomic radius
Nucleus
Beta-decay
Halogen
Chemical bond
Proton
Metal
Alkali Metal
Octet Rule
Neutron
Non-metal
Alkaline Earth metal
Ionic Bond
Electron
Metalloid
Noble gas
Non-polar (pure) covalent bond
Atomic Number
Electron configuration
Shielding Effect
Polar covalent bond
Mass Number
Orbital
Net nuclear attraction (Zeff)
Hydrogen bonding
Isotope
Chemical Groups (Families)
Ionization energy
Inter-molecular attraction
Radio-isotope
Chemical Period
Electronegativity
Intra-molecular attraction
2.
Complete the following chart:
Element
Atomic
Mass
Number of
Number of Electrons
Ion and its
Number of
Ionization Reaction
symbol
Number
Number
Neutrons
in Neutral Atom
charge
Electrons in Ion
Ag
108
20
20
35
17
18
22
39
20
60
47
65
30
Cu
34
28
34
79
80
45
3.
Referring to the chart in question #2,
a) Which atoms and ions are isoelectronic with each other?
b) Which atoms and ions are isotopes of one another?
4.
What one piece of information about an atom determines its chemical properties?
5.
What holds the electrons in an atom close to the nucleus?
6.
What happens to the potential energy of an electron when it moves further from the nucleus?
7.
One isotope of uranium is “U-238”. What does the number represent? How many neutrons does a U-238 atom have?
8.
Write electron configurations for neutral atoms of Zn, Ar, Ag and I.
2+
3-
9.
List any three ions or atoms that are isoelectronic with a Ca
ion. Repeat the question for a P
ion.
10. Use the concepts of net nuclear attraction and shielding effect to explain why:
a) atomic radius decreases from left to right across each period on the periodic table
b) electronegativity increases from left to right across each period on the periodic table (except for the Noble Gases)
c) metals become more reactive down each group
d) non-metals become less reactive down each group
11.
What are the trends on the Periodic Table for the following characteristics:
a) Ionization energy
b) Atomic Radius
c) Electronegativity
d) Reactivity of Metals; Reactivity of Non-metals
e) Metallic characteristics (same pattern as reactivity of metals)
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