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Gen Chem. (MCAT) > Ch.2 Bonding and Intermolecular forces > Flashcards

Ch.2 Bonding and Intermolecular forces Flashcards

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1
Q

What is a molecule?

A

any structure composed of multiple atoms

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2
Q

What is a compound?

A

a molecule that has atoms of more than one element connected together

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3
Q

When discussing nomenclature, how do you name binary compounds?

A

Ionic compounds - list cation first, then Anion second
Molecular compound - Arrange in order of electronegativity. (exception list carbon first, hydrogen after nitrogen)
Prefixes and suffixes are used in molecular compounds

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4
Q

What is an Ionic compound?

A

A metal and nonmetal molecule

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5
Q

What is a molecular compound?

A

It contains 2 nonmetals

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6
Q

In Ionic compounds why is it important that metal is identified with roman numerals?

A

Because it shows the oxidation state.

This allows us to determine how many electrons are being shared with another atom.

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7
Q

Forces that hold atoms together within a molecule are called?

A

Intramolecular forces

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8
Q

Forces that determine how molecules interact with each other are?

A

Intermolecular forces

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9
Q

What are the various types of Intramolecular forces?

A

Covalent, Ionic, and Metallic bonds

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10
Q

What is a covalent bond?

A

a bond formed between 2 nonmetals, by sharing valence electrons.
(they share electrons because their electronegativity lvl is similar)

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11
Q

What is a nonpolar covalent bond?

A

An element with the same (or similar) electronegativity are bonded together.

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12
Q

What is a polar covalent bond?

A

Atoms with a moderate difference in electronegativity are bonded together.

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13
Q

Covalent bonds have 2 different electronegativity values, what are they?

A

< .5 = nonpolar
.5 - 1.7 = polar
(greater than 1.7 = Ioninc bonds)

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14
Q

Since polar molecules unequally share electrons, a stable dipole forms. What is a dipole?

A

A dipole is a depiction of the vector of shared electrons.

A line with a plus is drawn.

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15
Q

What is an Ionic bond?

A

A complete transfer of one or more valence electrons (electronegativity must be >1.7).
Ionic bonding occurs between metal and nonmetal, and is stronger than covalent bonding.

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16
Q

Which is stronger covalent or Ionic?

A

Ionic bonding

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17
Q

Which type of force is stronger, intramolecular or intermolecular?

A

Intramolecular

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18
Q

What are the types of intermolecular bonding

A 
London dispersion
Dipole-dipole
Hydrogen
Ion-dipole
Ionic interactions
(in order from least to greatest)
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19
Q

What is a London dispersion force?

A

Occur when temporary dipoles arise by chance

larger structure will have a greater force

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20
Q

What is a Dipole-dipole interaction?

A

Occur between polar molecules.
It is a attractive force that occurs between the positive dipole of one polar molecule and the negative dipole of another.

21
Q

Explain hydrogen bonding

A

It is not true bonding
When hydrogen is attracted to lone pairs on nitrogen, oxygen, or fluorine. These molecules are highly electronegative and form strong bonds with hydrogen

22
Q

What are Ion-dipole forces?

A

These atrractions occur between an ion (charged molecule/atom) and a molecule with a dipole.

23
Q

The stronger intermolecular forces a compound has, the _________ it’s melting/ boiling point.

A

Higher

24
Q

When counting valence electrons a bond counts as how many electrons?

A

2

25
Q

Bond formation is considered a energy-________ reaction?

A

releasing (exothermic)

26
Q

Which molecules have exceptions to the octet rule, in which they can contain less?

A

hydrogen, Helium, and lithium = 2 electrons
Beryllium = 4 electrons
Boron = 6 electrons

27
Q

Which molecules have exceptions to the octet rule, in which they can contain more?

A

Atoms in the 3rd period and below.

Odd-electron molecules

28
Q

Typically metals (group 1 & 2) form _____ bonds with nonmetals (especially halogens). The electronegativity for this bind is?

A

Ionic bonds, electronegativity >1.7

29
Q

_________ compounds have a crystal lattice structure and high melting points due to the intramolecular forces.

A

Ionic

30
Q

__________ dissociates in an aqueous solution, which causes the solution the ability to conduct electricity.

A

Ionic compounds (electrolytes)

31
Q

Compared to ionic bonds, the elctronegativity difference for covalent bonds are

A

Smaller (.5)

32
Q

______ results from the complete donation or acceptance of electrons from an atom. While ______ share electrons.

A

Ionic bonds

Covalent bonds

33
Q

What are the most common polar and nonpolar covalent bonds?

A 
C-H = nonpolar
C-N = slightly polar
N-H = moderatly polar
O-H &amp; F-H = Highly polar
C- O = meaningful polar (less than H-O)
34
Q

What is a coordinate covalent bond?

A

a bond that forms when a set of lone pair electrons is shared with another atom without electrons to share.

35
Q

What is bond order?

A

number of bonds between two atoms

36
Q

Distinguish between sigma and pi bonds

A

Sigma bonds are the first single bonds to form (it represents the electrons shared between two molecules).
Pi bonds are each additional bonds

37
Q

Describe bond length

A

Distance between bonded atoms, or the distance between the nuclei of the atoms that are in the bond.
Bond length is inversely related to bond order.
single bond = furthest

38
Q

Describe bond energy

A

the energy required to break covalent bonds.

The higher the bond energy (triple) the harder to break. Bond energy is therefore directly related to bond order.

39
Q

What is formal charge?

A

The disparity between the number of valance electrons an atom should have (periodic table) and the number it actually has.

40
Q

What is the equation for formal charge?

A

FC = Valence elctrons - 1/2bonding electrons - Lone pairs of electrons

41
Q

Discuss hybridizations of orbitals

A 
1s 1p = 2 sp orbitals
1s 2p = 3 sp2 orbitals
1s 3p = 4 sp3 orbitals
Determine electron density around atom (bonds or lone pairs). 
If there are two region = sp
three regions = sp2
four regions = sp3
42
Q

What is the VESPR theory?

A

uses # of bonds and lone pairs to predict shape

43
Q

What are the various angles of VESPR?

A 
Bent (water) - 104.5
Trigonal pyramidal - 107
Tetrahedral - 109.5
Trigonal planar - 120
Linear - 180
44
Q

There are a few elements that do not follow the octet rule, what are they?

A

Hydrogen - only 1
Helium and lithium - maximum of two
Berilium - maximum of 4
Boron - max of 6

45
Q

When drawing a Lewis dot structure, which atom should be center?

A

The one with the lowest electronegativity

46
Q

After forming single bonds and calculating the remaining valence electrons for a Lewis dot structure, where should the remaining electrons go?

A

To the peripheral atoms

47
Q

Resonance structures differ in what why?

A

The distibution of electrons across the molecule

pi electrons should be shifted to different atoms

48
Q

Given a polyatomic transition metal, such as V(CO3)2, how do you balance?

A

Determine the charge on the polyatomic ion first (CO3) = CO3, 2-
Since there are 2 of these molecules, it brings the total charge to -4.
Than V must have the oxidation state of 4 (+4).
Vanadium (IV) carbonate

Gen Chem. (MCAT) (10 decks)

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