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Chemistry > 2 Chemical Bonding > Flashcards

2 Chemical Bonding Flashcards

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1
Q

What is a Chemical Bond?

A

The linkage or force which acts between 2 or more atoms to hold them together as a stable molecule.

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2
Q

Molecule is formed by the combination of

A

2 or more atoms

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3
Q

The concept of chemical bond is

A

Chemical Bonding

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4
Q

Reasons for chemical bonding between atoms:

A

The tendency of atoms to attain stable electronic configuration of the nearest noble gas.

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5
Q

2 Rules of stability

A

Octet rule and Duplet rule

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6
Q

2 methods of achieving chemical bonding

A
  1. Electron transfer

2. Electron sharing

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7
Q

Effect on the ease of formation of ionic compound with respect to:

  1. IP
  2. EA
  3. EN
A
  1. Inversely -> Cation
  2. Direct (Note: EA is only represented by -ve sign-> here absolute value is taken). -> Anion
  3. EN difference should be large.
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8
Q

Effect on the ease of formation of Covalent compound with respect to:

  1. IP
  2. EA
  3. EN
A

All the values should be high.

EN difference should be negligible.

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9
Q

Ionic Bond formation is due to _____.

A

Electrostatic force of electrostatic force of attraction between the ions.

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10
Q

Electrovalency

A

Number of electrons donated or accepted by the valence shell of an atom of an element.

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11
Q

____ may or may not exist independently. But ______ exist independently in solution.

A

Atoms; Ions;

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12
Q

In oxidation, there is
_____ in electrons or
____ in hydrogen or
______ in oxygen

A

Lose; Lose; Gain;

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13
Q

In reduction, there is
_____ in electrons or
____ in hydrogen or
______ in oxygen

A

Gain; Gain; Lose;

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14
Q

Ionic equation should have

A

Reduction and Oxidation equations

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15
Q

Electrovalent compounds involves ______ and ______. Covalent compounds involve _____ and _______.

A

Metal and Non-Metal.

Non-Metal and Non-Metal.

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16
Q

Number of bonds of each type is based on

A

the valency of the atoms

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17
Q

Covalent compound

A

Chemical bond formed due to the mutual sharing of electrons.
Between non-metallic elements

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18
Q

Covalency

A

Number of electron pairs which an atom shares with one or more atom of the same or different kind to achieve stable electronic configuration.

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19
Q

Non polar

A
  1. Shared pair of electrons are equally distributed between the 2 atoms.
  2. No charge seperation.
  3. Electrically neutral
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20
Q

Which type of bond has absolute symmetry?

A

Non-Polar covalent bonds

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21
Q

Polar

A
  1. Shared pair of electrons are unequally distributed between the 2 atoms.
  2. Charge seperation takes plalce.
  3. High electronegative -> slight negative charge.
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22
Q

If out of 2 atoms, one atom contributes x electrons. Then the bond is ____.

A

x covalent bond.

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23
Q

____ electrons in the outershell of each nitrogen atom are not involved in sharing during the formation of N2 molecules.

A

2

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24
Q

CCl4 has ____ single covalent bonds.

A

4

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25
Q

Is methane non-polar?

A

Yes

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26
Q

Does nitrogen molecule have a lone pair?

A

Yes. 1.

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27
Q

Does Methane molecule have a lone pair?

A

No

28
Q

Number of lone pairs in O2

A

2.

29
Q

Despite the C-Cl bond being polar, why not CCL4 not polar?

A

Due to symmetry, they canel out each other.

30
Q

What is lone pair of electrons?

A

Pair of electrons not shared with any other atom.

31
Q

An example of a stable positive ion?

A

Hydronium Ion.

32
Q

Number of lone pairs in hydronium ion?

A

1

33
Q

Addition of ___- to water results in the release of H ion.

A

Acids

34
Q

Number of lone pairs in ammonium ion?

A

0

35
Q

What is a coordinate bond?

A
  1. Type of covalency
  2. one of the combining atoms contribute both of the shared electrons.
  3. Bond; shared pair; both electrons from the same atom.
36
Q

Co-Ordinate bond doesnt come under covalency.

True or False.

A

False.

37
Q

Which bond has properties of both ionic and covalent?

A

Co-ordinate

38
Q

Another names for co-ordinate bonds

A

dative or co-ionic bond.

39
Q

Co-ordinate bond is also called co-coordinate bond.

True or false.

A

False.

40
Q

A compound which has Electrovalent and Covalent compound:

A

NaOH

41
Q

A compound which has Covalent and Co-ordinate compound:

A

CO and HNO3

42
Q

HNO3 has

A

A covalent and co-ordinate bond

43
Q

Compounds that has Ionic, Covalent and Co-ordinate bond

A

(NH4)Cl and K4 [Fe(CN)6]

44
Q

Ionic and Covalent compounds, exists in and why?

A

Crystalline hard solids -> Strong force of attraction between the ions, Gas, Liquids or Soft solids -> Weak force of attraction.

45
Q

Ionic and Covalent compounds, force of attraction:

A

Strong, Weak

46
Q

What forces are there between the ions/molecules in ionic and covalent compounda?

A

Electrostatic forces -> Between ions, Vander waal’s forces -> Between molecules

47
Q

Covalent compounds are gas if ______ and liquids or soft solids if _______.

A

Molecules are less; Molecules are more;

48
Q

Ionic and Covalent compounds, Volatility

A

Non-Volatile, Volatile

49
Q

Ionic and Covalent compounds, MP and BP. Reason.

A

HIGH -> Strong Electrostatic force of attraction between ions this large amount of energy to break the bond,
LOW -> Weak vaner waals force -> Less amount of energy.

50
Q

Ionic and Covalent compounds, Conduction of heat

A

Good

Bad

51
Q

Ionic compounds, Conduction of electricity

A

Solid state -> Non-Conductors
Liquid state -> Good conductors
Strong ES force keeps them in position. Weakened in molten and disappears in solution.

52
Q

The strong force of attraction _____ in molten state and _____ in solution state.

A

Weakened; Disappears;

53
Q

Covalent compounds, Conduction of electricity

A

Any state -> Non-conductors;
Only contains molecules and not ions. -> non-polar
Show charge seperation and seperate and dissosciate in H2O -> polar

54
Q

Ionic and Covalent compounds, Electrolysis

A

Ionic -> Yes. IN (liquid) or (aq) state.

Covalent -> No. But polar undergoes in (aq) state.

55
Q

Ionic and Covalent compounds, Solubility

A

Ionic -> Water;

Covalent -> Organic solvents; (non-polar);

56
Q

Organic solvents are always _______. (type)

A

Non-Polar.

57
Q

Ionic and Covalent compounds, Insolublity

A

Ionic -> Organic solvent

Covalent -> Water;

58
Q

What is Di-electric constant?

A

Capacity to weaken the force of attraction, resulting in free ions.

59
Q

Capacity to weaken the force of attraction, resulting in free ions.

A

Di-electric constant

60
Q

“LIKE DISSOLVES LIKE”

True or False.

A

TRUE!!!

61
Q

Water has a _____ di-electric constant. Organic solvents have a ____ di-electric constant.

A

High, Low.

62
Q

Reason for the solubility of non-polar compounds in organic compounds is

A

“Like Dissolves Like”

63
Q

Ionic and Covalent compounds, Reaction

A

Ionic -> High Speed IONIC Reactions. Rapidly regroup.

Covalent -> Slow speed molecular reactions. -> Slowly established.

64
Q

Ionic and Covalent compounds, Methods of charge creation

A

Ionic -> Electrolytic dissociation
Covalent -> Ionization.
on passage of current.

65
Q

Seperation of ions is called ____.

Formation of ions is called _________.

A

Electrolytic dissociation;

Ionization.

66
Q

Ionization happens in _____- state. Electrolytic dissociation happens in _____- state.

A

Solution state; Molten state;

67
Q

Electrolytic dissociation and Ionization occurs while there is a

A

Passage of electric current.

Chemistry (6 decks)

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