Day 2: Periodic Trends and Bonding

Question 1

Metals _____ electrons

Answer 1

lose

Question 2

Non-Metals_____ electron

Answer 2

gain

Question 3

Z-S =Zeff

Answer 3

Greater Zeff = smaller the atomic radius.

Electrons are held closer to nucleus

Question 4

Ionic radius increases

Answer 4

Down and to the left

France has wine & cheese = Fr biggest atomic radius

Question 5

Isoelectronic series

Answer 5

Most (+) smallest radius

Most (-) largest radius

Question 6

1st Ionization energy

Answer 6

Energy needed to remove an electron from the first shell
endothermic
oxidation
**Exceptions - B, O, N)

Question 7

Electron affinity

Answer 7

energy change associated with gaining an electron
Trend: to the right ( more (-))
Ionic bonding
Exothermic Reduction

Question 8

Electronegativity

Answer 8

Increases up and to the right
Covalent bonding
Exceptions: Be/N

Question 9

More polar bond

Answer 9

Bigger electronegativity difference

Question 10

Covalent network solids

Answer 10

Diamond & Quartz
non-metal with non-metal
Sharing e-

Question 11

Ionic (ionic crystals)

Answer 11

metal with non-metal
crystaline, high melting/boiling point
brittle

Question 12

Metalic (metalic lattices)

Answer 12

metal with metal
Valance e- loosely held
Electrical/thermally conductive 
Ductile- draw them into wires easily & malleable 
luster/shiny 
high melting/ boiling point

Question 13

Molecular

Answer 13

lower m.p. & b.p.

2 non-metals

Question 14

Lewis dot structures

Answer 14

***Exceptions: CH4, CO2, SF4)

Question 15

Polar covalent bonds

Answer 15

electrons shared by the atoms spend a greater amount of time, on the average, closer to the more electronegative atom, causing a dipole

Question 16

Coordinate covalent bonds

Answer 16

A covalent bond is formed by two atoms sharing a pair of electrons. The atoms are held together because the electron pair is attracted by both of the nuclei.

Lewis base & Lewis Acid

NH3 + HCl –> NH4Cl

Question 17

Exceptions to the octet rule

Answer 17

H -2 
Be- 4
B- 6
Al- 6
Can exceed octet- 3rd row or lower 
odd #

Question 18

Atoms on the left of the fisher projection

Answer 18

Axial position

Question 19

Atoms on the right of the fisher projection

Answer 19

Equatorial position

Lone pairs are put here due to large repulsion

Question 20

Hybirdization

Answer 20

Electrons are promoted (sp, sp2, sp3, sp3d, sp3d2)

Question 21

Electron domain - 2

non bonding pairs of e- = 0

Answer 21

sp
180 degrees
Electron Geometry -linear
Molecular Geometry- linear

Question 22

Electron domain - 3

non bonding pairs of e- = 0

Answer 22

sp2
120 degrees
EG- Trigonal planar
MG- Trigonal planar

Question 23

Electron domain - 3

non bonding pairs of e- = 1

Answer 23

sp2
120 degrees
EG- Trigonal planar
MG- Bent

Question 24

Electron domain - 4

non bonding pairs of e- = 0

Answer 24

sp3
109.5 dgrees
EG- Tetrahedral
MG-tetrahedral

Question 25

Electron domain - 4 | non bonding pairs of e- = 1

Answer 25

sp3 109.5 dgrees EG- Tetrahedral MG- Trigonal pyrimidal

Question 26

Electron domain - 4 | non bonding pairs of e- = 2

Answer 26

sp3 109.5 dgrees EG- Tetrahedral MG- Bent

Question 27

Electron domain - 5 | non bonding pairs of e- = 0

Answer 27

sp3d 90/120 degrees EG- Trigonal bypyrimidal MG- trigonal bypyrimidal

Question 28

Electron domain - 5 | non bonding pairs of e- = 1

Answer 28

sp3d 90/120 degrees EG- Trigonal bypyrimidal MG- see-saw

Question 29

Electron domain - 5 | non bonding pairs of e- = 2

Answer 29

sp3d 90/120 degrees EG- Trigonal bypyrimidal MG- T-shaped

Question 30

Electron domain - 5 | non bonding pairs of e- = 3

Answer 30

sp3d 90/120 degrees EG- Trigonal bypyrimidal MG- Linear

Question 31

Electron domain - 6 | non bonding pairs of e- = 0

Answer 31

sp3d2 90 degrees EG- Octahedral MG-Octahedral

Question 32

Electron domain - 6 | non bonding pairs of e- = 1

Answer 32

sp3d2 90 degrees EG- Octahedral MG-square pyrimidal

Question 33

Electron domain - 6 | non bonding pairs of e- = 2

Answer 33

sp3d2 90 degrees EG- Octahedral MG-square planar

Question 34

Single bond

Answer 34

sigma ( σ )- first bond in multiple bond is σ

Question 35

Multiple bonds

Answer 35

pi bonds ( π ) always p-p

Question 36

Inter molecular forces from strongest to weakest

Answer 36

``` Covalent Ionic Hydrogen bonding Dipole-dipole London dispersion forces- Van der Waals ```

Question 37

Hydrogen bonding

Answer 37

F, O, N bond with H2O | Bond required in a pure substance

Question 38

Dipole- Dipole

Answer 38

ion-dipole (equal in strength to H bonding) Dipole-induced pole Inter molecular force for polar molecules molecule is asymmetric, the bond dipole moments won't "cancel out" and the molecule will have a net dipole moment and the molecule is therefore polar.

Question 39

London Dispersal focres

Answer 39

Temporary or transient dipole. All molecules have these | More surface area, the greater the london dispersion forces (non-polar molecules)

Question 40

Higher intermolecular forces lead to

Answer 40

High b.p./ m.p., higher viscosity, high surface tension Lower vapor pressure