Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > L-2 Chemical Bonding > Flashcards

L-2 Chemical Bonding Flashcards

(75 cards)

Start Studying
1
Q

Why chemical bond formation occurs?

A

To achieve stability by achieving noble gas configuration (duplet or octet)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Define Chemical Bond

A

Force of attraction between any two atoms in a molecule to attain stability

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Define Ion

A

A charged particle which is formed due to gain or lose of one or more electrons by an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Metallic element is an

A

electropositive element (loses e and becomes cation)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Non metallic element is an

A

Electronegative element (gains e and becomes anion)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Ionic/Electrovalent bond

A

Bond formed by transfer of electrons from one atom of an electropositive element to one atom of another electronegative element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Force of attraction between cation and anion

A

Electrostatic force of attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Electrovalency

A

Number of electrons that an atom of an element gains or loses to form an Electrovalent bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Conditions for forming ionic bond

A

Low IE (cation formed easily)
High EA
More EN difference

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Most electropositive

A

G-1
(Caesium)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Most electronegative

A

G-17
(Fluorine)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Most ionic compound

A

CsF

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Bonds formed between metals and non metals are

A

ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Why are ionic compounds stable?

A

There exists a repulsive force between ions for like charges. Since electrostatic force of attraction between opposite charges is higher, it makes ionic compounds stable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Examples of electrovalent compounds

A

NaCl, MgCl2, CaO, KBr, CaCl2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Electropositive atom undergoes

A

oxidation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Electronegative atom undergoes

A

reduction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Why do oxidation and reduction occur simultaneously

A

because electrons lost by reducing agent must be gained by oxidising agent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Acceptor of electrons

A

Oxidising agent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Donor of electrons

A

Reducing agent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Define covalent bond

A

Bond formed between two or more atoms by mutual sharing of one or more pairs of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Sharing one pair of electrons

A

Single bond
eg- H2, Cl2, HCl, H2O, NH3, CCl4, CH4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Sharing two pairs of electrons

A

Double bond
Eg- O2, CO2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Sharing three pairs of electrons

A

Triple bond
Eg- N2, C2H4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Ethene
C2H4 one double bond and 4 single bonds
26
Ethyne
C2H2 One triple bond and two single bonds
27
Lone pair
pair of electrons not shared with any other atom
28
Bond pair
Bonded electrons
29
Covalency
Number of electrons taking part in formation of shared pairs to attain electronic configuration
30
Types of covalent bonds based on polarity
Polar and Non polar
31
Covalent bonds types based on shared pair of electrons
Single double and triple
32
Define polar covalent bond
When shared pair of electrons are not at equal distance between the two atoms Results in fractional positive and negative charges on them. Ionise in water
33
Polar covalent bond occurs due to
difference in EN shifts towards more EN element
34
Examples of polar covalent compounds
HCl, NH3, H2O, HF
35
Polar covalent molecules are also called
polar molecules
36
Highest EN difference in polar molecules
HF
37
Highest polarity in covalent molecules
HCl, HF, HBr, HI
38
Ionisation
Process by which covalent compounds are converted into ions
39
Process by which covalent compounds are converted into ions
Ionisation
40
Ionisation (in solution)
The fractional charges of polar covalent compounds are converted to complete charges and ions are produced. Process by which covalent compounds are converted into ions
41
Bond formed between two stoms 1- with same EN 2- with slightly different EN 3- with much EN difference is
1- Non-Polar 2- Polar 3- Ionic
42
Dipole molecule
Molecule that has both, slightly positive and slightly negative charge
43
Molecule that has both, slightly positive and slightly negative charge
Dipole molecule
44
Non polar covalent bond
When shared pair of electrons are equally distributed
45
When can bond formed between dissimilar atoms be non polar
If their EN difference is little and their structure permits the shared pair of electrons to attract equally the linked atoms and thus the molecule becomes symmetrical
46
Why are shared pair of electrons in methane at equal distance from carbon and hydrogen atoms?
Because the two have nearly equal Electronegativities
47
Favourable conditions for covalent bond
1- Non metals 2- High EA 3- High IE 4- High EN (in both) 5- Low EN difference
48
Ionic compounds are _____ conductors or electricity
good
49
Ionic compounds are non-volatile
High melting and boiling melts (strong force of attraction between oppositely charged ions, so large amount of energy is required to break the strong bonding force between ions)
50
Covalent compounds are volatile
Low boiling and melting points (weak forces of attraction between the binding molecules, less energy is required to break force of bonding)
51
Ionic compounds conduct electricity in which state?
Fused or aqueous state, not in solid state because forces weaken in fused or in solution state, so ions become mobile
52
Why are covalent compounds non conductors of electricity?
due to absence of free ions
53
In solution, ions become
mobile
54
In molten state, ions
dissociate
55
Polar covalent compounds ionise in their solutions and
act as electrolyte
56
Why do covalent compounds not dissociate?
because they do not have ions
57
Ionic compounds are soluble in _____\ but insoluble in _______
water, organic solvents water- polar covalent compound- decreases forces of attraction, resulting in free ions in aqueous solution
58
Covalent compounds are soluble in ______ but insoluble in ______
organic solvents, water organic solvents- non polar- dissolve non polar covalent compounds
59
Ionic compounds show _____ speed of reactions in aqueous state
rapid free ions are easily formed in different solutions, unite very fast forming compounds
60
covalent compounds show _____ speed of chemical reactions in aqueous state
slow old bonds broken and new bonds formed, thus reaction is slow between covalent compounds
61
Cause for chemical combination of atoms
tendency of atoms to acquire nearest noble gas configuration in their outermost shell and attain stability
62
Volatility
Ability to vaporise
63
Polar covalent compounds solubility in water
partially soluble due to partial charges on the bonded atoms
64
Define co-ordinate bond
Bond formed between two atoms by sharing a pair of electrons, provided entirely by one of the combining atoms but shared by both also called dative bond
65
Conditions for formation of covalent bond
One of the two combining atoms must have atleast one lone pair of electrons Another atom should be short of atleast a pair of electrons
66
Why is coordinate bond also called dative or co ionic bond
because it has properties of both covalent and ionic bonds
67
atom which provides the electron pair for formation of coordinate bond
donor
68
atom or ion which shares the donated electron pair
acceptor
69
shape of water molecule
wedge shaped
70
______ ion is a hydrated proton
Hydronium
71
Bonds in hydronium ion
One lone pair, two single covalent bonds and one coordinate bond
72
A compound having all three bonds
NH4Cl
73
Compounds having Electrovalent and covalent bonds
NaOH, CaCO3
74
Compound having covalent and coordinate bond
Sulphuric acid
75
Why does Hydroxyl ion have negative charge
When H+ ion is removed from water, the shared pair of electrons remains with Oxygen, as it is more electronegative

Chemistry (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions