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IB Chemistry > 4 - Bonding > Flashcards

4 - Bonding Flashcards

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1
Q

Types of bonds?

A

Covalent, dative covalent & ionic

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2
Q

Which bond forms between non-metals and metals?

A

Ionic

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3
Q

What happens to electrons in an ionic bond

A

They are either gained or lost

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4
Q

What happens to electrons in a covalent bond

A

They are shared between atoms

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5
Q

What is a covalent bond?

A

A shared paired of electrons make a covalent bond

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6
Q

How are covalent bonds formed?

A

Each atom in the bond shares one electron to form a bonding pair of electrons

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7
Q

How are dative bonds formed?

A

One of the atoms in the bond provides both electrons of the bonding pair

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8
Q

Examples of dative bonds

A

Ammonium, CO, nitric acid

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9
Q

Single bonds are always _________

A

Sigma bonds

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10
Q

Double bonds are made of ______ & ______

A

1 sigma and 1 pi bond

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11
Q

In which orbitals do sigma bonds occur?

A

s, p and hybrid orbitals

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12
Q

When do pi bonds form?

A

When two p orbitals overlap sideways

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13
Q

Which is stronger, pi or sigma bonds?

A

Sigma bonds are stronger. Pi bonds are further from the nucleus

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14
Q

Where is electron density in pi bonds?

A

Above and below internuclear axis

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15
Q

What are allotropes?

A

Different forms of the same element (e.g. graphite and diamond)

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16
Q

VSEPR Shape and angle: 2 bonding pairs

A

Linear, 180 (e.g. CO2)

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17
Q

VSEPR Shape and angle: 3 bonding pairs

A

Trigonal planar, 120 (e.g. Boron hydride)

18
Q

VSEPR Shape and angle: 4 bonding pairs

A

Tetrahedral (3D), 109.5 (e.g. CH4)

19
Q

VSEPR Shape and angle: 5 bonding pairs

A

Trigonal bypyramidal (3D), one plane at 180, others at 90 (e.g. Phosphorus pentaflouride)

20
Q

VSEPR Shape and angle: 6 bonding pairs

A

Octahedral (3D), all planes at 90 to each other (e.g. SF6)

21
Q

What is the effect of lone pairs on bond shapes?

A

Lone pairs are closer to nucleus, so they repel the bonding pairs, increasing bond length and shortening bond angle

22
Q

What does resonance state?

A

Resonance states that when there are multiple ways to draw Lewis diagrams, all possibilities are correct. (bonds can change to opposite sides)

23
Q

What does ozone do in the atmosphere?

A

Blocks out UVB & UVC

24
Q

Shape and angle: 4 bonding pairs, 2 lone pairs

A

Square planar, 90 (e.g. Xenon tetraflouride)

25
Q

Shape and angle: 4 bonding pairs, 1 lone pair

A

See-saw, 90 & 120

26
Q

What causes ozone to break down?

A

CFCs and NO

27
Q

Formal charge for most stable atoms?

A
  • Lowest possible

- Negative on electronegative atoms

28
Q

Types of hybridization

A

sp, sp2, sp3

29
Q

More the difference in electronegativity in a molecule, more the _______

A

Polarity

30
Q

Types of intermolecular forces with examples

A
  • van der Waals forces (I2, iodine)
  • Permanent dipole-dipole forces (HCl)
  • Hydrogen bonds (water)
31
Q

Rank intermolecular forces from strongest to weakest

A

1) Hydrogen bonds
2) Permanent dipole-dipole forces
3) Weakest: van der Waals forces

32
Q

What causes the strong attraction in hydrogen bonds?

A

A vast difference in electronegativity between H and O, N or F

33
Q

What factors cause van der Waals forces to increase?

A
  • Size of molecule increases

- Long, straight molecules have more van der Waals

34
Q

VSEPR Shape and angle: 2 bonding atoms, 1 lone pair

A

Bent (V-shaped),

35
Q

VSEPR Shape and angle: 1 bonding pair, 2 lone pairs

A

Linear, 180°

36
Q

VSEPR Shape and angle: 3 bonding atoms, 1 lone pair

A

Trigonal pyramidal,

37
Q

VSEPR Shape and angle: 2 bonding atoms, 2 lone pairs

A

Bent (V-shaped),

38
Q

VSEPR Shape and angle: 4 bonding atoms, 1 lone pair

A

See-saw, 90° & 120°

39
Q

VSEPR Shape and angle: 3 bonding atoms, 2 lone pairs

A

T-shaped, 90° & 120°

40
Q

VSEPR Shape and angle: 5 bonding atoms, 1 lone pair

A

Square pyramidal, 90° & 180°

41
Q

VSEPR Shape and angle: 4 bonding atoms, 2 lone pairs

A

Square planar, 90° & 180°

IB Chemistry (2 decks)

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