Final Exam Flashcards

1
Q

electron geometries

A
2 domains: linear
3 domains: trigonal planar
4 domains: tetrahedral
5 domains: trigonal bipyramidal
6 domains: octahedral
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2
Q

linear molecular geometry

A

2 situations-both 180 degrees

  1. 2 bonding groups, 0 lone pairs, nonpolar
  2. 2 bonding groups, 3 lone pairs, polar
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3
Q

trigonal planar molecular geometry(pairs, angle and polarity)

A

3 bonding pairs, 0 lone pairs, 120 degrees, nonpolar

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4
Q

bent molecular geometry(pairs, angle and polarity)

A

2 situations

  1. 2 bonded pairs, 1 lone pair, <120 degrees, polar
  2. 2 bonded pairs, 2 lone pairs, «109.5 degrees, polar
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5
Q

tetrahedral molecular geometry(pairs, angle and polarity)

A

4 bonded pairs, 0 lone pairs, 109.5 degrees, nonpolar

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6
Q

trigonal pyramidal molecular geometry(pairs, angle and polarity)

A

3 bonding pairs, 1 lone pair, <109.5 degrees, polar

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7
Q

trigonal bipyramidal molecular geometry(pairs, angle and polarity)

A

5 bonded pairs, 0 lone pairs, 120 degrees for equitorial bonds, 90 degrees for axial bonds, nonpolar

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8
Q

seesaw molecular geometry(pairs, angle and polarity)

A

4 bonded pairs, 1 lone pair, <120 degrees for equitorial, <109.5 degrees for axial bonds, polar

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9
Q

T-shaped molecular geometry(pairs, angle and polarity)

A

3 bonding pairs, 2 lone pairs, <90 degrees, polar

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10
Q

octahedral molecular geometry(pairs, angle and polarity)

A

6 bonding pairs, 0 lone pairs, 90 degres, nonpolar

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11
Q

square pyramidal molecular geometry(pairs, angle and polarity)

A

5 bonding pairs, 1 lone pair, <90 degrees, polar

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12
Q

square planar molecular geometry(pairs, angle and polarity)

A

4 bonding pairs, 2 lone pairs, 90 degrees, NONpolar

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13
Q

principle quantum number

A

n, defines energy levels

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14
Q

angular momentum quantum number

A
l, defines subshells, ranges from 0 to n-1
0=s
1=p
2=d
3=f
4=g
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15
Q

magnetic quantum number

A

ml, ranges from -l to l

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16
Q

spin quantum number

A

ms, value of + or - 1/2,

17
Q

ionization energy trend+equation

A

increases going up and to the right

X(g) = X^+(g) + e-

18
Q

effective nuclear charge definition+trend

A

increases going up and to the right

the charge an electron experiences from being attracted to the nucleus and from being repelled by other electrons

19
Q

electron affinity definition+equation+trend

A

energy change that occurs when an electron is added to a gaseous atom
X(g)+e- = X-(g)
Cl- has most electron affinity, halogens(17) have highest of all columns, then column 16 then column 1. Column 2 has 0 or almost 0 electron affinity.

20
Q

absorbing vs emitting energy

A

Absorption: increase n

Emission: decrease n

21
Q

ion dipole interaction

A

ions and polar solvents

22
Q

dipole dipole interactions

A

two polar molecules being attracted to each other

23
Q

H bond

A

H bonded to F, N or O

24
Q

lattice energy/enthalpy including reaction

A

🔼Hlattice, always negative, M+(g) + X-(g) = MX(s) whem neagtive, opposite if positive

25
🔼Hhydration
enthalpy change that occurds when gases are dissolved in water M+(g) + X-(g) = M+(aq) + X-(aq) **charges can differ
26
🔼Hsolution equation with lattice energy and enthalpy of hydration
🔼Hsolution=🔼Hhydration + 🔼Hlattice 🔼Hsolution is much smalle rin magnitude than 🔼Hhydration and 🔼Hlattice
27
🔼Hlattice trend
increases as charge difference increases, decreases as atomic radius increases
28
🔼Hhydratiobn trends
inverse relationship with atomic radius
29
difference between voltaic and electrolytic cell
not spontaneous, takes energy from surroundings, negatively charged cathode and postively charged anode
30
corrosion
a sacrificial anode with a lower reduction potential can be in contact with what is being corroded, and the corroding substance will become the cathode and no longer corrode
31
ionic compound properties
1. hard 2. brittle 3. high boiling/melting points 4. conduct electricity when dissolved in water
32
properties of covalent compounds
1. low melting/boiling points 2. brittle 3. poor conductors of heat and electricity evenw hen dissolved in water