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MCAT CHEMISTRY FLASHCARDS > MCAT CHEM CH. 5 > Flashcards

MCAT CHEM CH. 5 Flashcards

(73 cards)

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1
Q

Write the lewis dot structures of K, Si and Cl

A

Check Ch. 90 of chem book

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2
Q

What is a helpful way to calculate a proposed Lewis structure?

A

Calculate the formal charge

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3
Q

What is the equation for the formal charge?

A

FC = V - 1/2B - L

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4
Q

In the formal charge equation, what does V stand for?

A

Valence electrons

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5
Q

In the formal charge equation, what does B stand for?

A

Bonding electrons

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6
Q

In the formal charge equation, what does L stand for?

A

Number of lone-paired electrons

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7
Q

Based on formal charge, how do we know we have the correct lewis structure?

A

The one with the smallest formal charge

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8
Q

What is a resonance structure?

A

Two or more structures to accurately represent the reality of a molecule’s electron distribution

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9
Q

What is the bond dissociation energy?

A

The energy required to break a bond homolytically

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10
Q

What happens in a homolytic bond cleavage?

A

One electron of the bond being broken goes to each fragment of the molecule

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11
Q

What happens in a heterolytic bond cleavage?

A

Both electrons of the electron pair that make up the bod end up on the same atom, forming a cation and anion

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12
Q

What is a bond order? What’s the bond order of a single bond? Triple bond?

A

The number of bonds between adjacent atom; single bond=1, triple bond=3

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13
Q

What is the bond dissociation energies calculated in?

A

kcal/mol

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14
Q

What is the bond length calculated in?

A

angstroms, r A=10^-10m

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15
Q

What is the bond order trend?

A

The higher the bond order, the shorter and stronger the bond

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16
Q

How can bond order be compared?

A

Only be made for similar bonds

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17
Q

When comparing the same type of bond, the greater the s character in the hybrid orbitals….

A

The shorter the bond

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18
Q

Why are the s bond closer?

A

S-orbitals are closer to the nucleus than p-orbitals

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19
Q

How is the bond length of a p-orbital?

A

More directional hybrid orbital that is father from the nucleus and a longer bond

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20
Q

Based on bond strength, the longer the bond….

A

The weaker it is

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21
Q

Based on bond strength, the shorter the bond….

A

The stronger it is

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22
Q

What is a covalent bond?

A

The unpaired valence electrons are shared by both atoms

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23
Q

What is electronegativity basically?

A

How much an atom will “hog”the electrons that it’s sharing with another atom

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24
Q

What is a polar bond?

A

If the electron density between the two nuclei is uneven

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25
What is a non polar bond?
The electron density between the two nuclei is even
26
If the covalent bond is polar, what do we call the moment between the two atoms sharing the electrons?
Dipole moment
27
What is a coordinate covalent bond?
An atom will donate both of the shared electron in a bond
28
What is a Lewis base?
Molecule donates a pair of electrons
29
What can a Lewis base act as?
Ligand or a nucleophile
30
What is a Lewis acid?
Molecule that accepts a pair of electrons
31
What can a Lewis base act as?
Electrophile
32
What is an ionic bond?
The transfer of electrons to achieve a stable octet
33
How are the shapes of the molecules predicted?
Valence shell electro-pir repulsion theory
34
What determines the bond angles and orbital geometry of a molecule?
The total number of electrons groups on a central atom
35
What are the three simple bond angles type with no lone pairs?
Linear, trigonal planar, tetrahedral
36
What's the shape if an atom has 1 lone pair but 3 electron groups? 4 electron groups?
1. Bent 2. Trigonal pyramid
37
What's the shape if an atom has 2 lone pairs?
Bent
38
What concept is including in producing a set of composite, hybrid orbitals?
Orbital hybridization
39
How many lone pairs or attached atoms for an sp hybridization? What's the orbital geometry and bond angle?
2 in total, linear, 180 degrees
40
How many lone pairs or attached atoms for an sp^2 hybridization? What's the orbital geometry and bond angle?
3 in total, trigonal planar, 120 degrees
41
How many lone pairs or attached atoms for an sp^3 hybridization? What's the orbital geometry and bond angle?
4 in total, tetrahedral and 109.5 degrees
42
What is a sigma bond?
A bond consists of two electrons that are localized between two nuclei
43
What is a pi bond?
Parallel side to side alignment of two unhybridized p orbitals on adjacent atoms
44
How many sigma and pi bonds in the follow: 1. Single bond 2. Double bond 3. Triple bond
1. 1 sigma bond 2. 1 sigma, 1 pi 2. 1 sigma, 2 pi
45
What happens if the polar bonds cancel one another out?
Molecule as a whole is considered non polar and no dipole moment
46
What forces hold liquids and solids together?
Intermolecular forces
47
What are ion-dipole forces?
Polar molecules that are attracted to ions produce ion-dipole forces
48
What are dipole-dipolee forces?
Attraction between the positive end of one polar molecule and the negative end of another
49
What is a dipole-induced dipole force?
One molecule may induce a dipole in a neighboring non polar molecule
50
What is a London dispersion force?
An instantaneous dipole in a non polar molecule may induce a dipole in a neighboring non-polar molecule
51
What physical properties are affected by a molecule with stronger intermolecular forces?
Greater melting points, greater boiling points, greater viscosities, lower vapor pressure
52
The dipole forces, hydrogen bonding and London forces are all known as the....
Van Der Waals force
53
What are the two specific criteria's that must be fulfilled to be an H bond?
1. Molecule must have a covalent bond between H and either N, O or F 2. Molecule must have a lone pair of electrons on an N, O and F
54
How does the hydrogen bonds affect physical properties?
High boiling points
55
What is vapor pressure?
The pressure exerted by the gaseous phase of a liquid that evaporated from the exposed surface of the liquid
56
The weaker a substance's intermolecular forces, how is its vapor pressure?
The higher its vapor pressure and more easily it evaporates
57
What is a volatile liquid?
A liquid that easily vaporizes or has high vapor pressures
58
What physical property is vapor pressure dependent on?
Temperature; it increases with the temperature of the substance
59
What are ionic solids?
Held together by the electrostatic attraction between cations and anions in a lattice structure
60
What is the strength of the bond dependent on?
Primarily on the magnitudes of the ion charges
61
The greater the charge of the ions....
The stronger the force of attraction between the ions
62
The smaller the ions in an ionic solid....
The more they are attracted to each other
63
What is a network solid? How are the interactions?
Atoms are connected in a lattice of vocally bonds; all interactions between atoms are covalent bonds
64
What type of forces are there in a network solids?
Intermolecular forces
65
What are examples of network solids?
Diamond and quartz
66
What is different about metallic solids based on their electrons?
At east one valence electron per atom is not bound to any one particular atom and is free to move
67
What are the free valence electrons called in the metallic solids?
Conduction electrons
68
Due to the electrons being free and not bound to any particular atom, how does that impact the physical property of metallic solids?
Excellent conductors of electricity and heat, are malleable and ductile
69
Almost all metals are ____ at room temperature....
solids
70
What are molecular solids?
The particles at the lattice points of a crystal of a molecular solid are molecules
71
How is the melting and boiling points of molecular solids and why?
Low melting and boiling points because their force are weaker
72
How are molecular solids usually at room temperature?
Liquid or gases
73
Review molecular solids page 111
review molecular solids page 111

MCAT CHEMISTRY FLASHCARDS (4 decks)

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