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MCAT CHEMISTRY FLASHCARDS > MCAT CHEM CH. 5 > Flashcards

MCAT CHEM CH. 5 Flashcards

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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
Q

What is a non polar bond?

A

The electron density between the two nuclei is even

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26
Q

If the covalent bond is polar, what do we call the moment between the two atoms sharing the electrons?

A

Dipole moment

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27
Q

What is a coordinate covalent bond?

A

An atom will donate both of the shared electron in a bond

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28
Q

What is a Lewis base?

A

Molecule donates a pair of electrons

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29
Q

What can a Lewis base act as?

A

Ligand or a nucleophile

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30
Q

What is a Lewis acid?

A

Molecule that accepts a pair of electrons

31
Q

What can a Lewis base act as?

A

Electrophile

32
Q

What is an ionic bond?

A

The transfer of electrons to achieve a stable octet

33
Q

How are the shapes of the molecules predicted?

A

Valence shell electro-pir repulsion theory

34
Q

What determines the bond angles and orbital geometry of a molecule?

A

The total number of electrons groups on a central atom

35
Q

What are the three simple bond angles type with no lone pairs?

A

Linear, trigonal planar, tetrahedral

36
Q

What’s the shape if an atom has 1 lone pair but 3 electron groups? 4 electron groups?

A
  1. Bent 2. Trigonal pyramid
37
Q

What’s the shape if an atom has 2 lone pairs?

A

Bent

38
Q

What concept is including in producing a set of composite, hybrid orbitals?

A

Orbital hybridization

39
Q

How many lone pairs or attached atoms for an sp hybridization? What’s the orbital geometry and bond angle?

A

2 in total, linear, 180 degrees

40
Q

How many lone pairs or attached atoms for an sp^2 hybridization? What’s the orbital geometry and bond angle?

A

3 in total, trigonal planar, 120 degrees

41
Q

How many lone pairs or attached atoms for an sp^3 hybridization? What’s the orbital geometry and bond angle?

A

4 in total, tetrahedral and 109.5 degrees

42
Q

What is a sigma bond?

A

A bond consists of two electrons that are localized between two nuclei

43
Q

What is a pi bond?

A

Parallel side to side alignment of two unhybridized p orbitals on adjacent atoms

44
Q

How many sigma and pi bonds in the follow:

  1. Single bond
  2. Double bond
  3. Triple bond
A
  1. 1 sigma bond
  2. 1 sigma, 1 pi
  3. 1 sigma, 2 pi
45
Q

What happens if the polar bonds cancel one another out?

A

Molecule as a whole is considered non polar and no dipole moment

46
Q

What forces hold liquids and solids together?

A

Intermolecular forces

47
Q

What are ion-dipole forces?

A

Polar molecules that are attracted to ions produce ion-dipole forces

48
Q

What are dipole-dipolee forces?

A

Attraction between the positive end of one polar molecule and the negative end of another

49
Q

What is a dipole-induced dipole force?

A

One molecule may induce a dipole in a neighboring non polar molecule

50
Q

What is a London dispersion force?

A

An instantaneous dipole in a non polar molecule may induce a dipole in a neighboring non-polar molecule

51
Q

What physical properties are affected by a molecule with stronger intermolecular forces?

A

Greater melting points, greater boiling points, greater viscosities, lower vapor pressure

52
Q

The dipole forces, hydrogen bonding and London forces are all known as the….

A

Van Der Waals force

53
Q

What are the two specific criteria’s that must be fulfilled to be an H bond?

A
  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
Q

How does the hydrogen bonds affect physical properties?

A

High boiling points

55
Q

What is vapor pressure?

A

The pressure exerted by the gaseous phase of a liquid that evaporated from the exposed surface of the liquid

56
Q

The weaker a substance’s intermolecular forces, how is its vapor pressure?

A

The higher its vapor pressure and more easily it evaporates

57
Q

What is a volatile liquid?

A

A liquid that easily vaporizes or has high vapor pressures

58
Q

What physical property is vapor pressure dependent on?

A

Temperature; it increases with the temperature of the substance

59
Q

What are ionic solids?

A

Held together by the electrostatic attraction between cations and anions in a lattice structure

60
Q

What is the strength of the bond dependent on?

A

Primarily on the magnitudes of the ion charges

61
Q

The greater the charge of the ions….

A

The stronger the force of attraction between the ions

62
Q

The smaller the ions in an ionic solid….

A

The more they are attracted to each other

63
Q

What is a network solid? How are the interactions?

A

Atoms are connected in a lattice of vocally bonds; all interactions between atoms are covalent bonds

64
Q

What type of forces are there in a network solids?

A

Intermolecular forces

65
Q

What are examples of network solids?

A

Diamond and quartz

66
Q

What is different about metallic solids based on their electrons?

A

At east one valence electron per atom is not bound to any one particular atom and is free to move

67
Q

What are the free valence electrons called in the metallic solids?

A

Conduction electrons

68
Q

Due to the electrons being free and not bound to any particular atom, how does that impact the physical property of metallic solids?

A

Excellent conductors of electricity and heat, are malleable and ductile

69
Q

Almost all metals are ____ at room temperature….

A

solids

70
Q

What are molecular solids?

A

The particles at the lattice points of a crystal of a molecular solid are molecules

71
Q

How is the melting and boiling points of molecular solids and why?

A

Low melting and boiling points because their force are weaker

72
Q

How are molecular solids usually at room temperature?

A

Liquid or gases

73
Q

Review molecular solids page 111

A

review molecular solids page 111

MCAT CHEMISTRY FLASHCARDS (4 decks)

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