Midterm 2 Study

Question 1

What are paramagnetic atoms

Answer 1

Atoms that have more electrons spinning in one direction than the other

Question 2

What are diatomic atoms

Answer 2

Atoms with the same number of spin up and spin down electrons

Question 3

What is the shielding effect

Answer 3

• core electrons screen valence electrons from the attractive force of the nucleus
• Balance between attractive forces (e and p) result in sheilding

Question 4

What is orbital penetration

Answer 4

• Orbitals and sub shells define how close an electron can get to the nucleus
• The ability of an electron to get close to the nucleus is called penetration

Question 5

What are periodic trends in atomic radii

Answer 5

• Atomic radii increases from top to bottom and right to left
• Trends in atomic size result from differences in Zeff experienced by electrons in the outermost orbitals

Question 6

How atomic radii changes with the addition or loss of electron

Answer 6

With an addition
- Creates an anion, more e-e repulsion, larger radius
With a removal
- Creates anion, less e-e repulsion, smaller radius

Question 7

What is an isoelectronic species

Answer 7

Two elements or ions that have the same total number of electrons

Question 8

1st ionization energy trends

Answer 8

Ionization energy decreases from top to bottom and decreases from left to right
- As distance from nucleus to valence electron increases, the attraction lessens so its easier to pull apart

Question 9

What is electron affinity

Answer 9

• Energy released when an electron attaches to a molecule or atom to form an ion
• The more negative the an EA value is the more likely it is to gain an electron

Question 10

Trends in electron affinity

Answer 10

• Factors like Zeff and atomic size affect EA so trends are irregular
• Elements in group 16 and 17 have very high IE and highly negative EA, meaning they tend to lose e difficultly but attract them strongly
• Element in group 1 and 2 they have low IE and slightly negative EA meaning they lose e easily and attract them weakly
• Group 18 has very high IE and slightly positive EA and tend not to lose or gain e

Question 11

Electronegativity trends

Answer 11

• Electronegativity decreases from the top to the bottom and from left to right
• As atomic size increases the ability for a nucleus to attract electrons decreases

Question 12

Metallic characteristics

Answer 12

• A good heat and electricity conductor, malleability, shiny and tend to lose e in a reaction
• Metallic characteristics decrease as you move up and to the right
  ; increase in IE and more negative EA

Question 13

What are lattice energies

Answer 13

• Ionic bonding is attraction between positive and negative charged ions to form lattices
• Must know the structure of ionic compound to calculate lattice energy

Question 14

Trends in lattice energies

Answer 14

• Ions with a greater charge create higher energy lattices
• Smaller ions can get closer together, increasing the interaction between them (thus the lattice energy)

Question 15

What are bond strengths

Answer 15

• Its a measure of how much energy is required to break a bond
• Bond length decreases as bond strength increases

Question 16

Whats a non-polar covalent bond

Answer 16

• Bonding electrons shared equally
• No charges on atoms

Question 17

Whats a polar covalent bond

Answer 17

• Bonding electrons shared unequally
• Partial charges on atoms

Question 18

Whats an ionic bond

Answer 18

• Complete transfer of one or more valence electrons
• full charges on resulting ions

Question 19

What is Ionization Energy?

Answer 19

The minimum energy required to remove an electron

Question 20

2nd ionization energy

Answer 20

Second ionization energy: The energy it takes to remove an electron from a 1+ ion (meaning the atom has already lost one electron and now removing the second).

Question 21

1st ionization energy

Answer 21

first ionization energy of an element is the energy needed to remove the outermost, or highest energy, electron from a neutral atom in the gas phase.