Chemistry NAME: DATE: ___PERIOD:_____
Periodic Table Homework
1. Identify each property below as more characteristic of a metal or a nonmetal
Chemistry NAME: DATE: ___PERIOD:_____
a) A gas at room temperature
b) Brittle
c) Malleable
d) Poor conductor of electricity
e) Shiny
f) Ductile
Chemistry NAME: DATE: ___PERIOD:_____
2. Identify each element as a metal, metalloid, or nonmetal.
Chemistry NAME: DATE: ___PERIOD:_____
a) Fluorine
b) germanium
c) zinc
d) phosphorous
e) lithium
Chemistry NAME: DATE: ___PERIOD:_____
3. Give two examples of elements for each category.
Chemistry NAME: DATE: ___PERIOD:_____
a) noble gases
b) halogens
c) alkali metals
d) alkaline earth metals
Chemistry NAME: DATE: ___PERIOD:_____
4. Give the name and symbol for the element found at each of the following locations on the periodic table:
Chemistry NAME: DATE: ___PERIOD:_____
a) group 1; period 4
b) group 13; period 3
c) group 16; period 3
d) group 2; period 6
Chemistry NAME: DATE: ___PERIOD:_____
5. Where are the alkali metals, alkaline earth metals, halogens, transition metals, and the noble gases located in the periodic table?
6. Describe the relationship between the group number and the electron configuration of the elements in a group.
7. What trend in atomic radius do you see as you go down a group/family on the periodic table? What causes this trend?
8. What trend in atomic radius do you see as you go across a period/row on the periodic table? What causes this trend?
9. Circle the atom in each pair that has the largest atomic radius.
a) Al B b) S O c) Br Cl d) Na Al e) O F f) Mg Ca
10. Arrange the following elements in order of decreasing atomic size: sulfur, chlorine, aluminum and sodium. Explain if your arrangement demonstrates a periodic trend or a group trend
11. Indicate whether the following properties increase or decrease from left to right across the periodic table.
Chemistry NAME: DATE: ___PERIOD:_____
a) atomic radius
b) first ionization energy
c) electronegativity
d) electron affinity
Chemistry NAME: DATE: ___PERIOD:_____
12. Choose which statement about the alkali metals lithium and cesium is correct.
a) as the atomic number increases, the Electronegativity of the elements increases
b) as the atomic number increases, the first ionization energy of the elements decreases
c) as the atomic number increases, the atomic radius decreases
d) as the atomic number increases, the electron affinity increases
13. When a chlorine atom forms an ion its radius increases, but when a sodium atom forms an ion its radius decreases. Explain this apparent contradiction.
14. Choose which has the:
a) lowest first ionization energy: K, Na, Ca
b) largest radius: S2–, Cl–, Cl
c) highest electronegativity: As, Sn, S
d) smallest atom: Na, Li, Be
e) highest first ionization energy: C, N, Si
15. lithium, cesium, potassium, sodium, rubidium
a) Place the elements above in order from smallest atomic radius to largest atomic radius:
b) Place the elements above in order from smallest ionization energy to largest ionization energy:
c) Place the elements above in order from smallest electronegativity to largest electronegativity:
16. In each of the following pairs, circle the species with the higher ionization energy:
a) Li or Cs b)Cl or Ar c) Ca or Br d) Na+ or Ne e) B or Be
17. Determine which element you would expect to have the lowest first ionization energy.
Li Cs H He Ba
18. Identify which atom should have the largest value for the electron affinity:
He F Na Si Mn
19. Define ionization energy.
20. Is it easier to form a positive ion with an element that has high ionization energy or an element that has low ionization energy? Explain.
21. What trend in ionization energy do you see as you go down a group/family on the periodic table? What causes this trend?
22. Circle the atom in each pair that has the greater electronegativity.
a) Ca Ga b) Li O c) Cl S d) Br As e) Ba Sr f) O S
24. Ca Sr Ba Mg
a) most metallic?
b) least metallic?
c) lowest electronegativity?
d) highest ionization energy?
e) largest atomic radius?
f) which are non-metals?
g) list them in order form small to large.
h) would they gain or lost electrons to form ions? What charge would the ion have?
i) would the ion be larger or smaller than the atom?
j) lowest shielding effect?
k) would the ions be cations or anions?
l) what is the special name given to the group in which these elements belong?