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Chemistry HWAM > 2.2.2 Bonding > Flashcards

2.2.2 Bonding Flashcards

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1
Q

what is ionic bonding

A

Transfer of electrons resulting in a repeating pattern of oppositely charge ions.

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2
Q

what is the usual melting point of a ionically bonded substance and why

A

high due to strong electrostatic attraction

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3
Q

ionic bonding electrical conductivity

A

when molten/dissolved

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4
Q

what is covalent bonding

A

overlap of atomic orbitals to share a pair of electrons

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5
Q

do covalent bonded substances conduct electricity

A

no

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6
Q

octet rule

A

unpaired electrons pair up so their is always 8 electrons in outershell

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7
Q

why is the octet rule not always followed (2 point)

A

may not be enough electrons to react or more than 4 electrons may pair up

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8
Q

What are the 2 elements that can form less than 4 bonds/have less than 8 outer electrons. and why

A

Beryllium and boron. as they dont have enough electrons and will pair what’s available.

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9
Q

Example of a covalent bond with more than 8 outer electrons

A

SF6

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10
Q

What is a dative bond.

A

Covalent bond where both electrons come from the same atom.

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11
Q

How do dative bonds form

A

One atom that has a non-bonding pair of electrons and another atom that can accept 2 electrons.

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12
Q

What 2 things determine the 3-d structure of a molecule

A

Number of bonding pairs, number of non bonding pairs.

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13
Q

What is VSEPR

A

Valence shell electron pair repulsion theory

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14
Q

Angle and name of a molecule with 2 bonds

A

180° linear

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15
Q

Angle and name of a molecule with 3 bonds

A

120° trigonal planar

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16
Q

Angle and name of a molecule with 4 bonds

A

109.5° Tetrahedral

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17
Q

Angle and name of a molecule with 6 bonds

A

90° octahedral

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18
Q

How many ° are taken per lone pair of electrons

A

2.5°

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19
Q

Order of repulsion (electron pair types)

A

Bonded-bonded < Bonded-Lone < Lone-Lone.

20
Q

Angle and name of a molecule with 3 bonded pairs and 1 lone pair

A

107° pyramidal

21
Q

Angle and name of a molecule with 2 bonded pairs and 2 lone pairs of electrons

A

104.5° non-linear

22
Q

What is electronegativity

A

The ability to attract the bonding electron pair

23
Q

Top 3 electronegative elements in order

A

Nitrogen, Oxygen and fluorine. (NOF)

24
Q

2 factors that affect electronegativity and how,

A

1 atomic radius - radius increases-> distance from nucleus increases-> less attraction -> lower electronegativity
2 number of unshielded protons - more protons -> more attraction -> higher electronegativity

25
Q

What is the effect of full energy levels on electronegativity

A

Decreases

26
Q

What is a polar bond

A

An uneven distribution of electron density

27
Q

What causes polar bonds

A

When two have different electronegativity

28
Q

What are non-polar bonds

A

When electron density is shared evenly

29
Q

What causes non-polar bonds

A

When both atoms have identical electronegativity

30
Q

What symbol is used to show positive polar bond partial charge

A

δ+

31
Q

What symbol is used to show negative polar bond partial charge

A

δ-

32
Q

What is a Polar Molecule

A

A molecule with a large charge on one side that is not cancelled out. Generally unsymmetrical

33
Q

Are polar bonds covalent or ionic

A

Either

34
Q

What is a dipole

A

A molecule with 2 poles

35
Q

What are intermolecular forces

A

Forces that hold together molecules in a substance

36
Q

Are bonds broken when intermolecular forces are overcome

A

No (boiling water)

37
Q

What are London forces

A

Induced dipole dipole, when at any instant the electron of an atom find themselves at one end of atom a temporary charge is created. Another molecule close enough can have an induced charge from this dipole interaction.

38
Q

What increases London force strength

A

More electrons in molecule - larger induced dipole - stronger forces - more energy required to overcome.

39
Q

What are permanent dipole-dipole interactions

A

They act between permanent dipoles in different molecules.

40
Q

What are hydrogen bonds

A

A special case of permanent dipole dipole interactions that are stronger than London forces and permanent dipole dipole forces.

41
Q

what is required for a hydrogen bond to form

A

A hydrogen bonded to a electronegative atom (NOF) with a lone pair of electrons.

42
Q

waters 3 anomalous properties

A
  1. Hydrogen bonds push molecules further apart in open lattice structure ( when frozen)
  2. Molecules further apart in solid
  3. Solid ice is less dense than liquid water and floats.
43
Q

do simple molecular substances have a high or low melting/boiling point.

A

low due to weak intermolecular forces that can be easily overcome.

44
Q

what solvent will dissolve non-polar simple molecules

A

non-polar solvents

45
Q

what solvent will dissolve polar simple molecules

A

polar solvents

46
Q

Do simple molecular substances conduct electricity

A

no as there are no charged particles that are able to move.

Chemistry HWAM (13 decks)

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