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OAT- General Chemistry > Day 2: Periodic Trends and Bonding > Flashcards

Day 2: Periodic Trends and Bonding Flashcards

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1
Q

Metals _____ electrons

A

lose

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2
Q

Non-Metals_____ electron

A

gain

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3
Q

Z-S =Zeff

A

Greater Zeff = smaller the atomic radius.

Electrons are held closer to nucleus

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4
Q

Ionic radius increases

A

Down and to the left

France has wine & cheese = Fr biggest atomic radius

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5
Q

Isoelectronic series

A

Most (+) smallest radius

Most (-) largest radius

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6
Q

1st Ionization energy

A

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

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7
Q

Electron affinity

A

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

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8
Q

Electronegativity

A

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

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9
Q

More polar bond

A

Bigger electronegativity difference

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10
Q

Covalent network solids

A

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

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11
Q

Ionic (ionic crystals)

A

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

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12
Q

Metalic (metalic lattices)

A 
metal with metal
Valance e- loosely held
Electrical/thermally conductive 
Ductile- draw them into wires easily & malleable 
luster/shiny 
high melting/ boiling point
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13
Q

Molecular

A

lower m.p. & b.p.

2 non-metals

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14
Q

Lewis dot structures

A

***Exceptions: CH4, CO2, SF4)

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15
Q

Polar covalent bonds

A

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

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16
Q

Coordinate covalent bonds

A

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

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17
Q

Exceptions to the octet rule

A 
H -2 
Be- 4
B- 6
Al- 6
Can exceed octet- 3rd row or lower 
odd #
18
Q

Atoms on the left of the fisher projection

A

Axial position

19
Q

Atoms on the right of the fisher projection

A

Equatorial position

Lone pairs are put here due to large repulsion

20
Q

Hybirdization

A

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

21
Q

Electron domain - 2

non bonding pairs of e- = 0

A

sp
180 degrees
Electron Geometry -linear
Molecular Geometry- linear

22
Q

Electron domain - 3

non bonding pairs of e- = 0

A

sp2
120 degrees
EG- Trigonal planar
MG- Trigonal planar

23
Q

Electron domain - 3

non bonding pairs of e- = 1

A

sp2
120 degrees
EG- Trigonal planar
MG- Bent

24
Q

Electron domain - 4

non bonding pairs of e- = 0

A

sp3
109.5 dgrees
EG- Tetrahedral
MG-tetrahedral

25
Q

Electron domain - 4

non bonding pairs of e- = 1

A

sp3
109.5 dgrees
EG- Tetrahedral
MG- Trigonal pyrimidal

26
Q

Electron domain - 4

non bonding pairs of e- = 2

A

sp3
109.5 dgrees
EG- Tetrahedral
MG- Bent

27
Q

Electron domain - 5

non bonding pairs of e- = 0

A

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

28
Q

Electron domain - 5

non bonding pairs of e- = 1

A

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

29
Q

Electron domain - 5

non bonding pairs of e- = 2

A

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

30
Q

Electron domain - 5

non bonding pairs of e- = 3

A

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

31
Q

Electron domain - 6

non bonding pairs of e- = 0

A

sp3d2
90 degrees
EG- Octahedral
MG-Octahedral

32
Q

Electron domain - 6

non bonding pairs of e- = 1

A

sp3d2
90 degrees
EG- Octahedral
MG-square pyrimidal

33
Q

Electron domain - 6

non bonding pairs of e- = 2

A

sp3d2
90 degrees
EG- Octahedral
MG-square planar

34
Q

Single bond

A

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

35
Q

Multiple bonds

A

pi bonds ( π ) always p-p

36
Q

Inter molecular forces from strongest to weakest

A 
Covalent 
Ionic
Hydrogen bonding
Dipole-dipole
London dispersion forces- Van der Waals
37
Q

Hydrogen bonding

A

F, O, N bond with H2O

Bond required in a pure substance

38
Q

Dipole- Dipole

A

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.

39
Q

London Dispersal focres

A

Temporary or transient dipole. All molecules have these

More surface area, the greater the london dispersion forces (non-polar molecules)

40
Q

Higher intermolecular forces lead to

A

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

Lower vapor pressure

OAT- General Chemistry (7 decks)

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