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WorksheetsKAP Periodic Trends
Total questions: 30
Worksheet time: 32mins
Of the halogens, which has the smallest radius?
F
Br
He
At
Which of the following halogens has the greatest electronegativity?
Chlorine (Cl)
Bromine (Br)
Iodine (I)
Astatine (At)
Which group of elements has the lowest ionization energies?
Alkali Metals (Group 1)
Alkaline Earth Metals (Group 2)
Halogens (Group 17)
Noble Gases (Group 18)
What is a positively-charged ion which forms when an atom loses electrons?
atom
ion
cation
anion
What is a negatively-charged ion which forms when an atom gains electrons?
cation
anion
electron
ion
Which group of the periodic table is composed of inert (not reactive) gases?
If a potassium atom lost one electron, what would be the symbol for that ion?
Which element in period 4 has the highest electronegativity?
potassium
calcium
copper
bromine
The common charge on an atom in group 17 would be....
+1
+7
-7
-1
17
Consider the group 1A elements sodium (period 3), potassium (period 4), and rubidium (period 5). What would you predict about the ionization energies of these elements?
Na < K < Rb
Na > K > Rb
Rb < Na < K
Na = K = Rb
Which group 4A element has the highest ionization energy?
carbon
tin
silicon
lead
Copper is a common metal. Which of the following properties does this metal most likely have?
High conductivity, high malleability, and low luster
Low conductivity, low malleability, and low luster
High conductivity, high malleability, and high luster
Low conductivity, high malleability, and high luster
The elements in this family are soft, silvery, and very reactive with water.
Alkaline Earth Metals
Alkali Metals
Transition Metals
Lanthanides
This type of element is dull, brittle solids and gases, insulators, poor conductors of heat and electricity, as well as having low melting points.
metals
metalloids
nonmetals
Which of these elements in group 1A has the largest atomic radius?
cesium
rubidium
potassium
sodium
Electronegativity trends are the same as:
Atomic radius trends
Ionization energy trends
Both of these
None of these
Why does electronegativity decrease as you go down a group?
As you go down a group, the outer electrons are further away from the nucleus
As you go down a group, the nucleus is less able to attract electrons in a bond
Both of these
None of these
How does the following change when moving through the periodic table?
Effective nuclear charge across a period
Increases
Decreases
Stays the same
How does the following change when moving through the periodic table?
Shielding effect down a group
Increases
Decreases
Stays the same
