Question

1. which statement describes the general trends in electronegativity and ionization energy as the elements in period 4 are considered in order from k to kr?

a) electronegativity and first ionization energy both decrease.
b) electronegativity and first ionization energy both increase.
c) electronegativity increases, and first ionization energy decreases.
d) electronegativity decreases, and first ionization energy increases.

1. which trends are observed as each of the elements within group 14 on the periodic table is considered in order from top to bottom?

a) metallic properties and atomic radii both decrease.
b) metallic properties and atomic radii both increase.
c) metallic properties increase, and atomic radii decrease.
d) metallic properties decrease, and atomic radii increase.

Explanation:

For Question 17:

• Electronegativity trend: In a period (from left to right), as the atomic number increases, the nuclear charge increases while the number of electron shells remains the same. This leads to a stronger attraction for electrons, so electronegativity increases.
• First ionization energy trend: As we move from left to right in a period, the effective nuclear charge increases. It becomes more difficult to remove an electron, so first ionization energy also increases.

For Question 18:

• Metallic properties trend: As we move down group 14, the atomic size increases. The outermost electrons are more loosely held, and the elements tend to lose electrons more easily (a characteristic of metals), so metallic properties increase.
• Atomic radii trend: Down a group, new electron shells are added. The increase in the number of electron shells causes the atomic radius to increase.

Answer:

1. b) Electroncgativity and first ionization energy both increase.
2. b) Metallic properties and atomic radii both increase.