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Chemistry Final Flashcards

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1
Q

Isotopes

A

A= (atomic mass)(natural abundance)+(atomic mass)(natural abundance) [4.4% –> 0.44]

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2
Q

Ionic vs. Molecular

A

Ionic: [Metal + Nonmetal] High melting point & conductive
Molecular: [2 Nonmetals] Low melting point & not conductive

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3
Q

Anion vs. Cation

A

Anion [ ]- Adding a valence electron Cation [ ]+ Minus a valence electron

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4
Q

In an ionic compound, Metals are ___ and Non-metals are ___

A

Metals are cations (+)
Non-metals are anions (-)
*Cations always come first

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5
Q

The more shared electrons, the _____ + ____ the bond length is

A

The more shared electrons, the shorter and stronger the bond length is

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6
Q

When drawing cation/anion Lewis structures, pls remember to show

A

CHARGE

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7
Q

Steps to Building Lewis Structures

A
  1. Count v.e.
  2. Least electronegative atom in the middle
  3. Satisfy HONC + all Octets
  4. Are any exceptions applicable?
  5. Any Resonance
  6. Use formal charge to determine best Structure
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8
Q

Valence Shell Expansion

A

Elements in period 3 can fit more than octet in valence

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9
Q

Formal Charge

A

(V.E. of atom) - (1/2 of V.E. shared w/element) - (V.E. on element) = FC

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10
Q

Formal Charge (Choosing LS)

A

Most neutral charge should always be in the middle, no like charges next to each other
The molecule with the lowest charge state is the ideal molecule

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11
Q

Linear

A

2 bonds (not counting lone pairs) 180 degrees

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12
Q

Trigonal Planar

A

3 bonds (120)

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12
Q

Tetrahedral

A

4 bonds (109.5) (one dashed, one triangle)

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13
Q

Trigonal Bipyramidal

A

5 bonds (90, 120) (one dashed, one triangle)

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14
Q

Octahedral

A

6 bonds (90) (2 dashed, 2 triangle)

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15
Q

Angles are smaller than the ideal angle when…

A

When there are lone pairs on one side of a molecule being “fat” & taking up all the space, therefore crowding bonding groups on the other side. Double bonds create the same effect.
However symmetrical lone pairs cancel out and do not crowd

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16
Q

With resonance structures, ideal angles are always ______ to their actual angles

A

About the same

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17
Q

Molecules can only be polar if…

A

If their chemical bonds are polar (& don’t cancel out)

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18
Q

Zeff charge is…

A

Z (atomic #) - (# of core electrons)

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19
Q

Cations are ___ than their neutral element, because _______

A

Cations are smaller than their neutral atom, because loss of an electron shrinks the atom

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20
Q

Ionization Energy

A

Energy required to completely remove an electron from its shell

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21
Q

Electronegativity

A

The tendency of an atom to attract electrons towards itself

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22
Q

Hydrophilic

A

Polar & Water loving

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23
Q

Hydrophobic

A

Non-polar & Water fearing

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24
Kinetic Energy
The energy of an object in motion Higher temp = higher kinetic energy! Smaller Molar mass = higher energy!
25
The boiling point is higher if the ___, ____, & ____ is higher
Polarity, Branching area, & molar mass is higher
26
The 2 things that affect Solubility are....
Polarity I.M.F.s "Like dissolves like!" *big molecules are usually polar*
27
Kelvin to Celcius
K - 273.15 = C
28
1 Dalton = ...
1 g/mol
29
1 mol = ....
6.02x10^23
30
Interconversion!
2g = (x)mol/(x)g = (x)mol
31
The more ____, the higher the boiling point!
The more electrons, the higher the boiling point!
32
London Dispersion
(Non-polar) Affects evert molecule - Negative & positive parts of molecules attract, instantaneous dipole moment)
33
Dipole-Dipole
(Polar) Two polar molecules, positive end of one electronegative arrow attracts to the negative end of another
34
Hydrogen Bonding
Hydrogen donors & acceptors interlinking molecules
35
Hydrogen Donors
Hydrogens, but only hydrogens bonded to O, N, or F
36
Hydrogen Acceptors
Any O, N, or F
37
Ion-Dipole
Attraction between a charge ion (cation or anion), and a molecule w/a dipole (m+nm) + (nm +nm with dipole)
38
Solubility
Depends on 1. Polarity 2. IMFs "Like Dissolves Like!"
39
Scientific Notation!
<--- positive exponent! (larger) -----> negative exponent! (smaller)
40
Multiplying SI's
1. Rewrite the the problem to group the mantissas (1st number) and powers of 10 2. Multiply the mantissas 3. Multiply (add) the powers of 10
41
Dividing SI's
1. Rewrite the the problem to group the mantissas (1st number) and powers of 10 2. Divide the mantissas 3. Divide (subtract) the powers of 10
42
Interconversion!
1. Find a conversion factor 2. Use conversion factor to write a unit ratio 3. Multiply the measurement!
43
single bonds: double bonds: triple bonds:
1 sigma 1 sigma + 1pi 1 sigma + 2 pi
44
the lower the orbital the...
better it is at screening electrons from the influence of the nucleus
45
sp3
4 sigma bonds 0 pi bonds (4 electron groups)
46
sp2
3 sigma bonds 1 pi bonds (3 electron groups)
47
sp
2 sigma bonds 2 pi bonds (2 electron groups)
48
sp3-
3 sigma bonds 0 pi bonds
49
sp2+
3 sigma bonds 0 pi bonds
50
Solving for Reactant (What mass of A is consumed w/5g of B given)
1. Balance chemical equation 2. 5g/20g(given)--> .25mol 3. .25 molB --> .25mol A 4. .25mol A (given A) --> 3.75gA!
51
Calculate the molar mass by
finding the sum of the molar masses, multiplied by the number of atoms in that element!
52
Solving for reactant, from mols
1. (mols produced)/(mols consumed) 2. (mols produced)/(given) = answer!
53
Finding mol ratio
1. (atoms of x)/(atoms of y) 2. (given mol)(x/y) = x!
54
moles ---> mass
(molar mass)(moles given)
55
Could half of ____ reactant react??
1. Calculate how much product would be produced if half the initial amount of reactant reacted 2. Calculate how much of the otherrr reactant will be consumed if half the initial reactant will be consumed 3. Is it more or less than the given of the second reactant?
56
Calculate the limiting reactant
1. Balance equation 2. g-->mol of both products, using molar mass and given grams 3. which is smaller? *remember to double atomic mass if ex: Cl2
57
THEORETICAL YIELD!
1. Balance equation 2. Find limiting reactant 3. lr(mols. of what we want/mols of lr)=x 4. (x)(molar mass of element we want) =theoretical yield!
58
% yield
(actual yield)/(theoretical yield)x100%
59
Heat released/or absorbed
How many mols of NO2 react? (grams given)/(molar mass NO2) = mol NO2 (△given)55.3/2mol NO2 (mol NO2) 2.0824(55.3/2) = 57.578! exo (-): released endo (+): absorbed
60
Calculating heat of reaction from bond energies
1. CH4 + 2O2 ---> CO2 + H2O 2. Draw Lewis structures to find amount of bonds 3. Break - Make = Answer!
61
(E) (v) (λ) (h) Plancks Constant (c) Speed of light
(E) Energy (v) Frequency (λ) Wavelength (h) 6.626x10^-34 (c) 299792458
62
n: l: ml:
n: shape of orbital (principal quantum #) l: type of orbital (The principal angular momentum quantum number) ml: orientation of suborbital (Magnetic quantum number)
63
L0: L1: L2:
L0: Sphere L1: Hourglass L2: 4-Leaf Clover
64
sp3d
5 electron groups
65
sp3d2
6 electron groups
66
Calculating wavelength from KJ/MOL
Given/Avogadros # = ___x10^-19 | ___x10^-19/Plancks = ____x10^14 | 299792458/____x10^14 = 0.0000 --> 000.0nm
67
Calculating wavelength from KHZ
299792458/given kHz 980 kHz ---> 9.8x10^5 = 0.0000... ---> 000.0nm
68
Calculating Frequency
299792458/given wavelength 18.5 tHz ---> 1.85x10^13 = 0.0000... ---> 00.0um
69
Formula for wavelength
λ=c/v
70
Formula for frequency
c/λ
71
Electromagnetic Spectrum In order of DECREASING wavelength
Gamma Rays X-rays Ultraviolet Visible (400-700) Infrared Microwave Radio
72
As wavelength _____, frequency and energy _____
As wavelength decreases, frequency and energy increase!
73
Finding Wavelength Graphically
absorbed (upwards arrow) emitted (downwards arrow) higher state - lower state = energy of photon (ex: 200) (Plancks)(299792458)/2.00x10^19 =0.00 ----> 000.0nm
74
Atomic Ionizeability
Energy needed to ionize an atom decreases as you go DOWN the pt
75
S: P:
S: 1 boob P: 2 boobs
76
On a graph, the highest probability contains the ______, and the lowest probability contains the _____
The highest probability contains the LEAST energy, and the lowest probability contains the MOST energy
77
Hybridization Chain
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10, 5p6, 6s2, 4f14, 5d10, 6p6, 7s2, 5f14, 6d10, 7p6!

Chemistry (2 decks)

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