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chemistry a level > Chemical bonding > Flashcards

Chemical bonding Flashcards

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1
Q

Ionic bonding

A

the electrostatic force between cations and anions in an ionic crystal lattice

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2
Q

Covalent bonds

A

formed when the outer electrons of two atoms are shared

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3
Q

How are atoms between molecules kept together ?

A

by strong covalent bonds

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4
Q

Van der Waals’ forces

A

weak forces between molecules

-> intermolecular forces

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5
Q

Types of Van der Waals’ forces

A
  • dipole
  • permanent dipole-permanent dipole ( pd-pd forces )
    -hydrogen bonding
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6
Q

London dispersion forces ( dipole )

A

instantaneous dipole-induced dipole ( id-id ) forces

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7
Q

Hydrogen bonding

A

stronger form of pd-pd force

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8
Q

How are ions formed

A

by the gain or loss of electrons in atoms

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9
Q

Positive ions ( Cations )

A

when an atom loses one or more electrons

-> mostly metals

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10
Q

Negative ions ( Anions )

A

when an atom gains one or more electrons

-> mostly non-metals

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11
Q

Lattice

A

a regularly repeating arrangement of atoms, molecules or ions in 3-D throughout the whole crystal structure

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12
Q

Ionic bond

A

the electrostatic attraction between oppositely charged ions ( cations & anions )

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13
Q

Electrovalent bond

A

Ionic bond

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14
Q

Dot-and-cross diagram

A

a diagram showing the arrangement of the outer-shell electrons in an ionic/ covalent element/compound

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15
Q

Dot-and-cross diagram structure

A
  • outer shells only
  • the charge of the ion is spread only, by using square brackets
  • the charge on each ion, shown on the right-hand top corner
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16
Q

Covalent bonding

A

when two non-metals share one or more pairs of electrons

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17
Q

Single covalent bond / bond pair

A

the electrostatic attraction between the nuclei of two atoms and a shared pair of electrons

represented by a single line between atoms

ex : Cl-Cl

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18
Q

Lone pair

A

pairs of electrons in the outer shell of an atom that are not involved in bonding

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19
Q

Double covalent bonding

A

two shared pairs of electrons bonding 2 atoms together

represented by a double line between atoms

ex : O=O

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20
Q

Dative covalent bonding /
Co-ordinate bonding

A

the sharing of electrons between two atoms where both the electrons in the bond come from the same atom

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21
Q

Needs for dative bonding

A
  • one atom has a lone pair of electrons
  • a second atom to have an unfilled orbital to accept the lone pair
    -> electron deficient
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22
Q

Electron deficient

A

an atom/molecule that has less than its usual share of electrons

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23
Q

Bond energy

A

the energy required to break one mole of a particular covalent bond in gaseous state

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24
Q

Bond length

A

the distance between the nuclei of two covalently bonded atoms

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25
Q

Shape & bond angle of a covalently bonded molecule depends on :

A
  • number of pairs of electrons around each atom
  • whether these pairs are lone pairs or bonded pairs
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26
Q

VSEPR

A

Valence Shell Electron Pair Repulsion Theory

27
Q

Shapes of molecules

A
  • linear ( v-shape )
  • trigonal planar
  • tetrahedral
  • trigonal bipyramid
  • octahedral
28
Q

Linear

A
  • 2 electron pairs
  • 180°
29
Q

Trigonal planar

A
  • 3 electron pairs
    120°
30
Q

Tetrahedral

A
  • 4 electron pairs
  • 109.5
31
Q

Trigonal bipyramid

A
  • 5 electron pairs
  • 90°, 120°
32
Q

Octahedral

A
  • 6 electron pairs
  • 90°
33
Q

Molecular orbital

A

combined orbital formed when the atomic orbitals in the formation of a covalent bond overlap

  • contains 2 electrons
34
Q

Hybridisation

A

the mixing of atomic orbitals

35
Q

Sigma bonds ( σ )

A

formed from end-on overlap of atomic orbitals

36
Q

Pi bonds ( π )

A

formed from sideways overlap of atomic orbitals

37
Q

Metallic bonding

A

the electrostatic attraction between positive ions and delocalised electrons

38
Q

Delocalised electrons
( mobile electrons )

A

electrons that are not associated with any particular atoms

39
Q

Delocalised electrons in metals

A

move throughout the metallic structure between the metal ions when a voltage is applied

40
Q

Strength of metallic bonding increases with :

A
  • increasing positive charge on the ions in the metal lattice
  • decreasing size of metal ions in the lattice
  • increasing number of mobile electrons per atom
41
Q

Properties of metals :

A
  • high MP & BP
  • conduct electricity
  • conduct heat
42
Q

Metals as an electricity conductor

A

when a voltage is applied to a metal, electric current flows through it because the mobile electrons are free to move

43
Q

Metals as a heat conductor

A
  • mainly due to the vibrations passed from one metal ion to the next
  • partly due to the movement of delocalised electrons
44
Q

Electronegativity

A

the power of a particular atom that is covalently bonded to another atom to attract the bonding pair of electrons towards itself

45
Q

Pattern of electronegativity from Group 1-17

A
  • increases across a period
  • increases down a group
46
Q

Most electronegative element

A

Fluorine

47
Q

Order of the most electronegative elements

A

Br < Cl < N < O < F

48
Q

Factors influencing electronegativity :

A
  • atomic radius
  • nuclear charge
  • shielding
49
Q

Scale of electronegativity values

A

Pauling electronegativity
-> Np

50
Q

electronegative difference is high ( ≥ 2.0 )

A

ionic

51
Q

electronegative difference is low ( < 1.0 )

A

covalent

52
Q

Non-polar molecules

A
  • electronegativity values of the two atoms forming a covalent bond are the same
  • equally shared pair of electrons
53
Q

Polar molecule ( dipole )

A
  • different electronegative values between two atoms forming a covalent bond
  • electron distribution is asymmetric
54
Q

In molecules containing more than 2 atoms, we have to take into account :

A
  • the polarity of each bond
  • the arrangement of each bonds in the molecule
55
Q

Polar bonds

A

the electron pair in the atom is drawn towards the atom having the larger electronegativity, making one end of the molecule slightly positive compared to the other

56
Q

Induced

A

one molecule brings about an attractive or repulsive effect on the other

57
Q

id-id forces

A
  • Instantaneous dipole - induced dipole forces
  • weakest intermolecular attractive force
  • dipoles not permanent
  • London dispersion forces
58
Q

id-id forces increase with :

A
  • increasing number of electrons & protons in the molecule
  • increasing the number of contact points between the molecules
59
Q

pd-pd forces

A
  • attractive intermolecular forces which result from permanent dipoles in a molecule
60
Q

For hydrogen bonding to happen, the molecules must have :

A
  • a H atom atom bonded to a highly electronegative atom
  • another highly electronegative atom with a lone pair of electrons
61
Q

Hydrogen bond

A
  • strongest type of intermolecular force
  • weaker than covalent bonds
  • strong type of pd-pd force
62
Q

The average number of hydrogen bonds formed per molecules depends on :

A
  • number of hydrogen atoms attached to F,O or N
  • the number of lone pairs present on the F,O or N
63
Q

Properties of water :

A
  • high enthalpy change of vaporisation & BP
  • Surface tension & viscosity

chemistry a level (32 decks)

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