3.2 Physical Properties - 1
SWBAT:
Understand trends in atomic radius, ionic radius, first ionisation energy, electron affinity and electronegativity across a period
Understand trends in atomic radius, ionic radius, first ionisation energy, electron affinity and electronegativity down a group
Understand that elements in the same group have similar chemical properties and show a gradual variation in physical
properties
Describe some reactions of elements in group 1 and group 17
Describe the changes from basic to acidic oxides across a period
Write equations for the reactions of oxides with water and predict the acidity of the resulting solutions
Part 1 – Atomic and Ionic Radii
1. Based on the position of the elements on the Periodic Table, place the following in order from smallest to largest. Also,
explain why the trend exists.
a. Mg, Mg2+
f. Li+, B3+, Be2+
b. O2-, O
g. S, Cl, I-, Cl-, S2-
c. Ba, Mg, Sr, Ca
h. Ar, Cl-, K
d. O2-, Na+, F-
i. F-, Na+, Ne
e. H+, H, H-
j. S2-, Ca2+, K+, Ar, Cl-
2. Explain why it is difficult to measure atomic and ionic radii for the noble gases.
Part 2 – First Ionization Energy
1. Define first ionization energy.
2. Write the equation for the first ionization of the following atoms.
a. Mg
b. P
c.
Ca
d. F
3. Based on the position of the elements on the Periodic Table, determine the element with the highest ionization energy
using > or <.
a. Li
Na
c. C
Sn
e. B
Be
b. S
Cl
d. Al
Mg
f.
P
c.
N
S
Part 3 – Electron Affinity
1. Define electron affinity.
2. Write the equation for the first electron affinity of the following atoms.
a. O
b. Cl
Part 4 – Electronegativity
1. Define electronegativity.
2. Based on the position of the elements on the Periodic Table, determine the element with the highest electronegativity
using > or <.
a. Li
Na
c. N
O
e. K
Rb
b. Mg
K
d. P
N
f. F
Na
3. Explain why there are no electronegativity values for the noble gases.
Part 5 – Periodic Trends Summary
Determine if the following statements are true or false. If false, correct the statement so that it is true.
a. A gallium atom is smaller than an aluminum atom, but aluminum has a higher first ionization energy.
b. Arsenic has a higher first ionization energy and electronegativity than phosphorus.
c.
Tin has a higher first ionization energy and electronegativity than indium.
d. Br- is bigger than Br, but Te2- is smaller than Te.
e. Chlorine has a higher electronegativity than sulfur but a lower electronegativity than fluorine.
Part 6 – Group 1 Elements
1. Explain why the melting point decreases moving down the group.
2. Determine which element will be more reactive.
a. K
Na
b. Rb
Cs
c.
K
d. Li
Rb
K
3. Write the equation for each reaction.
a. K with O2
b. Li with H2O
c.
Rb with O2
d. Na with H2O
Part 7 – Group 17 Elements
1. Explain why the melting point increases moving down the group.
2. Write the balanced chemical equation (with state symbols) when the following halogens and alkali metals react.
a. K and Br2
b. Na and I2
c.
Li and F2
d. K and Cl2
3. Determine if a displacement reaction (competition for the extra e-) will occur between the following
species. If a reaction will occur, write the balanced equation (with state symbols). If no reaction will occur,
write ‘no reaction’.
a. Br- and Cl2
d. I- and Br2
b. Cl- and I2
c.
-
Cl and Br2
e. Br- and I2
f.
F2 and Cl-
4. Describe and explain what you will see if chlorine gas is bubbled through a solution of…
• NaBr
• NaF
Part 8 – Oxides of Period 2 and 3
1. Identify the following oxides as being either acidic, basic or amphoteric.
a. Na2O
c. MgO
b. P4O10
d. SO3
2. Write an equation for the following oxides when placed into water.
a. Na2O
b. SO3
c.
P4O10
d. CO2
e. MgO
f.
NO2
e. CaO
f.
NO2