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?
k) would the ions be cations or anions?
l) what is the special name given to the group in which these elements belong?

Question

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?
k) would the ions be cations or anions?
l) what is the special name given to the group in which these elements belong?

Accepted Answer

### Problem 22 (Electronegativity Comparison)
#### a) Ca vs Ga
# Explanation:
## Step1: Recall electronegativity trend
Electronegativity increases across a period (left to right) and decreases down a group (top to bottom). Ca is in group 2, period 4; Ga is in group 13, period 4.
## Step2: Compare positions
Since Ga is to the right of Ca in the same period, Ga has greater electronegativity.
# Answer: Ga

#### b) Li vs O
# Explanation:
## Step1: Recall electronegativity trend
Li is in group 1, period 2; O is in group 16, period 2.
## Step2: Compare positions
O is to the right of Li in the same period, so O has greater electronegativity.
# Answer: O

#### c) Cl vs S
# Explanation:
## Step1: Recall electronegativity trend
Cl is in group 17, period 3; S is in group 16, period 3.
## Step2: Compare positions
Cl is to the right of S in the same period, so Cl has greater electronegativity.
# Answer: Cl

#### d) Br vs As
# Explanation:
## Step1: Recall electronegativity trend
Br is in group 17, period 4; As is in group 15, period 4.
## Step2: Compare positions
Br is to the right of As in the same period, so Br has greater electronegativity.
# Answer: Br

#### e) Ba vs Sr
# Explanation:
## Step1: Recall electronegativity trend
Electronegativity decreases down a group. Ba is below Sr in group 2.
## Step2: Compare positions
Sr is above Ba, so Sr has greater electronegativity.
# Answer: Sr

#### f) O vs S
# Explanation:
## Step1: Recall electronegativity trend
Electronegativity decreases down a group. S is below O in group 16.
## Step2: Compare positions
O is above S, so O has greater electronegativity.
# Answer: O

### Problem 24 (Ca, Sr, Ba, Mg - Group 2 Elements)
#### a) Most metallic?
# Explanation:
## Step1: Recall metallic character trend
Metallic character increases down a group (as atomic size increases, losing electrons becomes easier).
## Step2: Identify the lowest element
Among Ca, Sr, Ba, Mg, Ba is the lowest in group 2.
# Answer: Ba

#### b) Least metallic?
# Explanation:
## Step1: Recall metallic character trend
Metallic character decreases up a group (smaller atomic size, harder to lose electrons).
## Step2: Identify the highest element
Among Ca, Sr, Ba, Mg, Mg is the highest in group 2.
# Answer: Mg

#### c) Lowest electronegativity?
# Explanation:
## Step1: Recall electronegativity trend
Electronegativity decreases down a group (larger atoms attract electrons less).
## Step2: Identify the lowest element
Ba is the lowest in group 2, so it has the lowest electronegativity.
# Answer: Ba

#### d) Highest ionization energy?
# Explanation:
## Step1: Recall ionization energy trend
Ionization energy decreases down a group (electrons are farther from nucleus, easier to remove).
## Step2: Identify the highest element
Mg is the highest in group 2, so it has the highest ionization energy.
# Answer: Mg

#### e) Largest atomic radius?
# Explanation:
## Step1: Recall atomic radius trend
Atomic radius increases down a group (more electron shells).
## Step2: Identify the lowest element
Ba is the lowest in group 2, so it has the largest atomic radius.
# Answer: Ba

#### f) Which are non - metals?
# Explanation:
## Step1: Recall group 2 elements' nature
Ca, Sr, Ba, Mg are all in group 2 (alkaline earth metals), which are metals.
## Step2: Conclusion
None of Ca, Sr, Ba, Mg are non - metals.
# Answer: None (all are metals)

#### g) Order from small to large (atomic radius)?
# Explanation:
## Step1: Recall atomic radius trend
Atomic radius increases down a group. The order from top (smallest) to bottom (largest) in group 2 is Mg, Ca, Sr, Ba.
## Step2: Arrange accordingly
So the order from small to large is Mg < Ca < Sr < Ba.
# Answer: Mg, Ca, Sr, Ba

#### h) Gain or lose electrons? Charge?
# Explanation:
## Step1: Recall group 2 elements' valence electrons
Group 2 elements have 2 valence electrons.
## Step2: Determine electron behavior
To achieve a stable octet, they lose 2 electrons. When they lose 2 electrons, they form ions with a +2 charge.
# Answer: Lose electrons; Charge of +2

#### i) Ion vs atom size?
# Explanation:
## Step1: Recall ion size trend for metals
When a metal loses electrons, it forms a cation. The cation has fewer electron shells or less electron - electron repulsion, so it is smaller than the atom.
## Step2: Conclusion for group 2 ions
Group 2 elements form cations (lose electrons), so the ion is smaller than the atom.
# Answer: Smaller

#### k) Cations or anions?
# Explanation:
## Step1: Recall cation/anion definition
Cations are positively charged ions (formed by losing electrons), anions are negatively charged (formed by gaining electrons).
## Step2: Determine for group 2
Group 2 elements lose electrons to form +2 ions, so they are cations.
# Answer: Cations

#### l) Special name of the group?
# Explanation:
## Step1: Recall group 2 name
Elements in group 2 of the periodic table are called alkaline earth metals.
## Step2: Conclusion
The group of Ca, Sr, Ba, Mg is called alkaline earth metals.
# Answer: Alkaline earth metals

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Problem 22 (Electronegativity Comparison)

a) Ca vs Ga

Step1: Recall electronegativity trend

Step2: Compare positions

Step1: Recall electronegativity trend

Step2: Compare positions

Step1: Recall electronegativity trend

Step2: Compare positions

Answer:

b) Li vs O