Chapter 1 and 2 Problems

Question 1

incomplete 3 d shell

Answer 1

transition metal

Question 2

complete 3 p shell

Answer 2

inert gas

Question 3

uncompleted 3 p shell

Answer 3

halogen

Question 4

completed 4 s shell

Answer 4

alkaline earth metal

Question 5

incomplete 4 s shell

Answer 5

alkali metal

Question 6

whats the conversion for nanometers to meters

Answer 6

10^9

Question 7

Ionic Characteristics

Answer 7

electrostatic attraction between oppositely charged ions
(metal and non-metal)

Question 8

Covalent Characteristics

Answer 8

electron sharing between 2 atoms to gain stableness
(non-metal and non-metal)

Question 9

Metallic Characteristics

Answer 9

positive cores are shielded and glued together by a sea of valence electrons
(metal and metal)

Question 10

hydrogen bonding requirements

Answer 10

• must be bonded to either oxygen or nitrogen
• fluorine is an exception

Question 11

Melting point Hierarchy

Answer 11

primary bonding:
ionic > covalent > metallic
secondary bonding:
hydrogen > di-pole > van der waals

lower molecular weight = lower melting point?

Question 12

Exceptions to filling s shell before d shell

Answer 12

Copper and chromium

Question 13

amount of s, p, d and f spots

Answer 13

S: 1 spot (2 electrons)
P: 3 spots (6 electrons)
D: 5 spots (10 electrons)
F: 7 spots (14 electrons)

Question 14

Left side vs Right side Periodic Table

Answer 14

Left Side: Electropositive
Right Side: Electronegative

Question 15

What are attraction and repulsion forces dependent on?

Answer 15

r: separation of interatomic distance

Question 16

FN Equation

Answer 16

FN = FA + FR

which means
FA = -FR

Question 17

Energy Equation

Answer 17

E = EA + ER

Question 18

Bonding Capacity depending on states

Answer 18

solid = large bonding capacity (high melting point)
liquid = intermediate bonding capacity ( mid melting point)
gaseous = low bonding capacity (low melting point)

Question 19

Intermolecular vs Intramolecular

Answer 19

Intra = primary bonds (holds atoms together within a molecule)
Inter = secondary bonds (bond molecules together)

Question 20

metals, ceramic and polymer bonding

Answer 20

Metals: metallic bonding
Ceramics: ionic bonding
Polymers: covalent bonding

Question 21

Metal Characteristics

Answer 21

• good conductivity
• high strength
• high stiffness
• ductility

Question 22

Ceramic Characteristics

Answer 22

Compounds of metallic and non-metallic elements
- non-conductive
- high hardness
- high strength
- high melting point
- very brittle

Question 23

Wave-like Characteristics of electrons

Answer 23

• electrons are in orbitals defined by a probability
• each orbital at discrete energy levels is determined by quantum numbers

Question 24

Energy Levels/Shells

Answer 24

K- Shell 1s
L - Shell 2s 2p
M - Shell 3s 3p 3d
N - Shell 4s

Question 25

Valance Shell

Answer 25

If any level isnt filled, it makes the whole shell the valance shell.
(Example: 1s^2 2s^2 2p^2 L Shell is valance)

Question 26

sp3 vs sp2

Answer 26

sp3
-s and p levels completely combine
sp2
- s and p shells don’t combine fully

Question 27

VSEPR Theory

Answer 27

-double and triple bonds have stronger repulsive forces than single bonds
- lone pairs also distort angles