Match the group to the type of ions they form
Column A
1.
Group 1A:
Group 1A
2.
Group 2A:
Group 2A
3.
Group 3A:
Group 3A
4.
Group 4A:
Group 4A
5.
Group 5A:
Group 5A
6.
Group 6A:
Group 6A
7.
Group 7A:
Group 7A
8.
Group 8A:
Group 8A
Column B
a.-3
b.+1
c.+3
d.-2
e.0
f.-1
g.+4/-4
h.+2
1. Group 1A: b. +1
2. Group 2A: h. +2
3. Group 3A: c. +3
4. Group 4A: d. -2
5. Group 5A: f. -1
6. Group 6A: e. 0
7. Group 7A: g. +4/-4
8. Group 8A: e. 0
Column A
1. Group 1A: b.+1
2. Group 2A: h.+2
3. Group 3A: c.+3
4. Group 4A: e.0
5. Group 5A: f.-1
6. Group 6A: d.-2
7. Group 7A: g.+4/-4
8. Group 8A: e.0
To match the groups in Column A to the type of ions they form in Column B, we need to know the valence electrons of each group. Valence electrons are the electrons in the outermost energy level of an atom and determine the chemical properties of an element.
1. Group 1A: This group includes elements like hydrogen (H), lithium (Li), sodium (Na), and potassium (K). They have 1 valence electron and tend to lose that electron to form a +1 ion. So, the answer is b, +1.
2. Group 2A: This group includes elements like beryllium (Be), magnesium (Mg), calcium (Ca), and strontium (Sr). They have 2 valence electrons and tend to lose those electrons to form a +2 ion. So, the answer is h, +2.
3. Group 3A: This group includes elements like boron (B), aluminum (Al), and gallium (Ga). They have 3 valence electrons and tend to lose those electrons to form a +3 ion. So, the answer is c, +3.
4. Group 4A: This group includes elements like carbon (C), silicon (Si), and germanium (Ge). They have 4 valence electrons and can either lose or gain electrons, depending on the situation. However, they usually do not form ions and instead form covalent bonds by sharing electrons with other atoms. So, the answer is e, 0.
5. Group 5A: This group includes elements like nitrogen (N), phosphorus (P), and arsenic (As). They have 5 valence electrons and tend to gain 3 electrons to complete their octet and form a -3 ion. So, the answer is a, -3.
6. Group 6A: This group includes elements like oxygen (O), sulfur (S), and selenium (Se). They have 6 valence electrons and tend to gain 2 electrons to complete their octet and form a -2 ion. So, the answer is d, -2.
7. Group 7A: This group includes elements like fluorine (F), chlorine (Cl), and bromine (Br). They have 7 valence electrons and tend to gain 1 electron to complete their octet and form a -1 ion. So, the answer is f, -1.
8. Group 8A: This group includes elements like helium (He), neon (Ne), and argon (Ar). They have 8 valence electrons and are already stable with a full octet. Therefore, they do not form ions. So, the answer is g, +4/-4 (as these elements can gain or lose electrons to fulfill the octet in reactions).
Matching the groups from Column A to the type of ions they form in Column B:
1. Group 1A: b, +1
2. Group 2A: h, +2
3. Group 3A: c, +3
4. Group 4A: e, 0
5. Group 5A: a, -3
6. Group 6A: d, -2
7. Group 7A: f, -1
8. Group 8A: g, +4/-4