Question

ionization energy
choose the element with the higher first ionization energy from each pair:
a. br or bi b. na or rb c. as or at d. p or sn

Explanation:

To solve for the element with the higher first ionization energy in each pair, we use the trend of ionization energy in the periodic table: ionization energy generally increases from left to right across a period and decreases from top to bottom within a group.

Part (a): Br or Bi

Step 1: Locate the elements in the periodic table

• Bromine (Br) is in period 4, group 17.
• Bismuth (Bi) is in period 6, group 15.

Step 2: Apply the ionization energy trend

• Moving from left to right across a period, ionization energy increases. Moving down a group, ionization energy decreases.
• Br is in a higher period (closer to the top) and further to the right in the periodic table compared to Bi. So, Br has a higher first ionization energy.

Part (b): Na or Rb

Step 1: Locate the elements in the periodic table

• Sodium (Na) is in period 3, group 1.
• Rubidium (Rb) is in period 5, group 1.

Step 2: Apply the ionization energy trend

• Both elements are in group 1. As we move down a group, ionization energy decreases because the outermost electrons are further from the nucleus and experience less effective nuclear charge.
• Na is above Rb in group 1, so Na has a higher first ionization energy.

Part (c): As or At

Step 1: Locate the elements in the periodic table

• Arsenic (As) is in period 4, group 15.
• Astatine (At) is in period 6, group 17.

Step 2: Apply the ionization energy trend

• As is in a lower period (closer to the top) than At. Also, as we move down a group, ionization energy decreases. Even though At is in group 17 (to the right of group 15), the effect of being in a lower period (down the group) has a more significant impact on decreasing ionization energy. So, As has a higher first ionization energy.

Part (d): P or Sn

Step 1: Locate the elements in the periodic table

• Phosphorus (P) is in period 3, group 15.
• Tin (Sn) is in period 5, group 14.

Step 2: Apply the ionization energy trend

• P is in a higher period (closer to the top) and further to the right (group 15 vs group 14 for Sn) in the periodic table.
• Moving from left to right across a period, ionization energy increases, and moving up a group (decreasing period number) increases ionization energy. So, P has a higher first ionization energy.

Final Answers:

a. $\boldsymbol{\text{Br}}$
b. $\boldsymbol{\text{Na}}$
c. $\boldsymbol{\text{As}}$
d. $\boldsymbol{\text{P}}$

Answer:

To solve for the element with the higher first ionization energy in each pair, we use the trend of ionization energy in the periodic table: ionization energy generally increases from left to right across a period and decreases from top to bottom within a group.

Part (a): Br or Bi

Step 1: Locate the elements in the periodic table

• Bromine (Br) is in period 4, group 17.
• Bismuth (Bi) is in period 6, group 15.

Step 2: Apply the ionization energy trend

• Moving from left to right across a period, ionization energy increases. Moving down a group, ionization energy decreases.
• Br is in a higher period (closer to the top) and further to the right in the periodic table compared to Bi. So, Br has a higher first ionization energy.

Part (b): Na or Rb

Step 1: Locate the elements in the periodic table

• Sodium (Na) is in period 3, group 1.
• Rubidium (Rb) is in period 5, group 1.

Step 2: Apply the ionization energy trend

• Both elements are in group 1. As we move down a group, ionization energy decreases because the outermost electrons are further from the nucleus and experience less effective nuclear charge.
• Na is above Rb in group 1, so Na has a higher first ionization energy.

Part (c): As or At

Step 1: Locate the elements in the periodic table

• Arsenic (As) is in period 4, group 15.
• Astatine (At) is in period 6, group 17.

Step 2: Apply the ionization energy trend

• As is in a lower period (closer to the top) than At. Also, as we move down a group, ionization energy decreases. Even though At is in group 17 (to the right of group 15), the effect of being in a lower period (down the group) has a more significant impact on decreasing ionization energy. So, As has a higher first ionization energy.

Part (d): P or Sn

Step 1: Locate the elements in the periodic table

• Phosphorus (P) is in period 3, group 15.
• Tin (Sn) is in period 5, group 14.

Step 2: Apply the ionization energy trend

• P is in a higher period (closer to the top) and further to the right (group 15 vs group 14 for Sn) in the periodic table.
• Moving from left to right across a period, ionization energy increases, and moving up a group (decreasing period number) increases ionization energy. So, P has a higher first ionization energy.

Final Answers:

a. $\boldsymbol{\text{Br}}$
b. $\boldsymbol{\text{Na}}$
c. $\boldsymbol{\text{As}}$
d. $\boldsymbol{\text{P}}$