Unit 2 Paper 2 questions

Question 1

Explain why sulfur has lower 1st ionization energy than oxygen and phosphorus.

Answer 1

Sulfur lower than O
- Same group but lower
- The lower the element the higher the ionization energy
- Energy increases across a period Sulfur has a lower energy than P
- b/c d orbitals are half - filled in P

Question 2

Describe the acid - base character of the oxides of period 3 elements Na to Ar.

Answer 2

..answer

Question 3

For sodium oxide and sulfur trioxide write balanced equations to illustrate their acid-base character

Answer 3

• Na2O(s) + H2O(l) –> 2NaOH(aq)
• SO3(s) + H2O –> H2SO4 (aq)
  !CHECK!

Question 4

What is the meaning of electronegativity?

Answer 4

A measure of the ability of an atom to attract electrons in a covalent bond

Question 5

State and explain the trend in electronegativity across period 3 from Na to Cl

Answer 5

Electronegativity increases b/c nuclear charge increases and atomic radii decreases

Question 6

Why would Cl2 rather than Br2 react more vigorously with a solution of I?

Answer 6

B/c reactivity decreases down the group b/c the atomic radii increases and traction for the outer electrons decreases.
- The larger the electronegativity difference the vigorous the reaction

Question 7

What is ionization energy?

Answer 7

The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms in their ground state

Question 8

Write an equation, including state symbols, for the process occuring when measuring the first ionization of Al

Answer 8

Al(g) –> Al(g)+1 + e-

Question 9

Why is the 1st ionization energy of Mg greater than Na?

Answer 9

B/c :
- Atomic radii decreases
- # of protons increase but not shielding or energy levels
Meaning Mg is higher b/c it has larger Zeff and smaller atomic radius