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Chemistry > Bondings > Flashcards

Bondings Flashcards

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1
Q

Ionic Bonding

A

? The electrostatic attraction between oppositely charged ions

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2
Q

Metallic Bonding

A

? Electrostatic attraction between delocalised electrons and positively charged metal ions

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3
Q

Covalent bonding

A

? Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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4
Q

Dative Covalent bond

A

? One atom donates both of the electrons in the covalent bond. They are equivalent to other covalent bonds.

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5
Q

Electronegativity

A

? The power of an atom to attract a pair of electrons in a covalent bond.
? The measure of the attraction of a bonded atom for the pair of electrons in the covalent bond.

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6
Q

Non polar covalent bonds

A

? Forms when the atoms (made of the same element) have identical electronegativities

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7
Q

Polar covalent bonds

A

? Forms when the elements in the bond have different electronegativities (of around 0.3-1.7)

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8
Q

Intramolecular forces

A

? forces within molecules

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9
Q

Intermolecular forces

A

? forces between molecules

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10
Q

Hydrogen bonding

A

? Occurs between a hydrogen atom and a lone pair of electrons on a very electronegative atom. (H-O, H-N, H-F)

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11
Q

Melting point

A

? Is the temperature a species starts to melt which the same temperature the species starts to freeze

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12
Q

Boiling point

A

? Is the temperature a species starts to boil which is the same temperature the species starts to condense

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13
Q

Valence Shell electron pair repulsion theory (VSEPR)

A

? The shape adopted by a single molecule or ion is that which keeps repulsive force to a minimum.

electrons in the outer shell of atoms arrange themselves as far apart as possible to minimise repulsion

decrease by 2.5 degrees

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14
Q

The shape of: 2 electron pairs - both bonding pairs

A

Linear, 180 degrees

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15
Q

The shape and angle of 3 electron pairs - 3 bonding pairs

A

Trigonal planar 120 degrees

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16
Q

The shape and angle of 3 electron pairs - 2 bonding pairs & 1 lone pair

A

Bent, around 119 degrees

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17
Q

Order of strengths of repulsion

A

Lone-lone > Lone-bonding > bonding-bonding

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18
Q

4 electron pair; 4 bonding pairs

A

Tetrahedral, 109.5 degrees

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19
Q

4 electron pairs; 3 bonding pair, & 1 lone pair

A

Trigonal pyramidal, 107 degrees

20
Q

4 electron pairs; 2 bonding pairs & 2 lone pairs

A

Bent, 104.5 degrees

21
Q

How many degrees does a lone pair reduce the bond angle by?

A

Approximately 2.5 degrees

22
Q

5 electron pairs; 5 bonding pairs

A

Trigonal Bipyramidal, 90/120 degrees

23
Q

5 electron pairs; 4 bonding pairs& 1 lone pair

A

Sawhorse, <90/<120 Degrees

24
Q

6 electron pairs; 6 bonding pairs

A

Octahedral, 90 degrees

25
Q

6 electron pairs; 5 bonding pairs & 1 lone pair

A

Square pyramidal, < 90 degrees

26
Q

Properties of Ionic Bonding

A

High MP/BP - oppositely charged ions
Conduct electricity -molten/aqueous
Brittle - - layers repel

27
Q

Properties of metallic bonding

A

Conduct electricity - delocalised electrons

Malleable, ductile - layers can slide over each other without repulsion.

28
Q

The strength of metallic bond depends on ….

A

Charge, ↑charge greater attraction

Size, smaller the metal ions closer the electrons is to the (+) nucleus, greater attraction

29
Q

Trends in electronegativity down a group and across a period

A

Down a group - Electronegativity ↓, as atomic radius ↑, ↑shielding, ↑ distance between the nucleus and the bonding pair, ↓attraction.

Across a period, electronegativity ↑, atomic radius ↓, ↑nuclear charge, ↑ attraction between the nucleus and the bonding pair.

30
Q

Types of intermolecular forces

A 
Van der waals 
- Very weak (occurs at split seconds) 
Permanent dipole 
- if aligned correctly attraction
Hydrogen Bonding 
- HN,HF,HO
31
Q

How does hydrogen bonding give water unique properties?

A
  • surface tension
  • excellent solvent
  • liquid at room temp
  • highly polar molecule
  • High MP/BP
32
Q

What structure does ice have ?

A

tetrahedral. When ice melts, structures collapse slightly, molecules come close, then move a little apart as ↑ E.
Water has maximum density at 4 degrees

33
Q

Formula for sulfate

A

SO4(2-)

34
Q

Formula for hydroxide

A

OH-

35
Q

formula for carbonate

A

CO3(2-)

36
Q

formula for ammonium

A

NH4+

37
Q

How can you represent co-ordinate bonds

A

Using an arrow

38
Q

Describe the properties of diamond

A
  1. Very high melting point
  2. Strong - tetrahedral structure
  3. Non-conductor of electricity - no delocalised electron
39
Q

Properties of graphite

A
  1. high MP
  2. Soft - hexagonal
  3. conductor of electricity
40
Q

Properties of silicon dioxide/silica

A
  1. High MP
  2. Strong - silicon is joined to 4 oxygen
  3. non-conductor of electricity
41
Q

What is a symmetric molecule

A

A symmetric molecule (all bonds identical and no lone
pairs) will not be polar even if individual bonds within
the molecular ARE polar.

42
Q

describe how the electron distribution in a covalent bond between elements with different electronegativities will be unsymmetrical?

A

Permanent dipole-dipole forces occurs between polar molecules
•It is stronger than Van der Waals and so the compounds have higher boiling points
•Polar molecules have a permanent dipole. (commonly compounds with C-Cl, C-F, C-Br H-Cl, C=O bonds) •Polar molecules are asymmetrical and have a bond where there is a significant difference in
electronegativity between the atoms.

43
Q

How do you show that a bond is polar

A

Partial charges

44
Q

Can you explain why some molecules with polar bonds do not have a permanent dipole?

A

This is due to the symmetry in some polar molecules,so the dipoles cancel each other out. For example, water is a polar molecule, however, as water is negatively charged on one side and positively charged on the other, the charges cancel each other out

45
Q

Can you explain the importance of hydrogen bonding in the low density of ice and the anomalous boiling points of compounds?

A

Ice is less dense than water because the orientation of hydrogen bonds causes molecules to push farther apart, which lowers the density.
The anomalously high boiling points of H2O,
NH3 and HF are caused by the hydrogen
bonding between the molecules

Chemistry (11 decks)

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