Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Introductory Chemistry Flashcards > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

what does each dot represent

A

Each dot represents one valence
electron

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

what is special about noble gases

A

noble Gases have filled outer shells

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

what can lewis dot structures be used for

A

Lewis Dot structures or the valance electrons can predetermine the
way elements react or combine together to form compounds

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

molecular compounds

A

Held together with covalent bonds
Atoms share electrons with other atoms
Electrons-mutual sharing of a pair of
electrons

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

how is an ionic bond created

A

Ionic Bond: Results From the Force of Attraction Between a Cation and an Anion

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

ionic compounds

A

Atoms gain or lose electrons to
become ions

Cations with a positive charge and
Anions with negative charge
Attracted by oppositely charged ions

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

how is an ionic compound created

A

Ionic compound results when a metal reacts with a non-metal
Electrons are transferred.

Ionic compounds have a definite ratio of one kind of ion to another

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

define an ionic bond

A

Ionic bond: Electrostatic attraction between a positive ion (cation) and a
negative ion (anion)

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

how is ionisation energy calculated

A

Ionisation energy is calculated in the gaseous state (kJ/mol)

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

Applying a particular amount of energy atoms can gain or loose electrons
to form their respective ions

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

what is the octet rule

A

The octet rule: atoms gain or lose electrons to achieve an inert gas configuration

There is a degree of stability observed with a
filled valence shell:

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

what happens to the ionisation energy as we move across the periodic table

A

The ionisation energy increases as we move across the row in the periodic table.
This can be explained by the forces associated with the increasing positive nature
of the nucleus.

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

what are group-1 elements

A

alkali metals

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

what do the alkali metals have in common and what is the characteristic ionic charge

A

They all have one electron in their outer shell or they would like to lose one electron to have 8 electrons in their outer shell (achieve Noble Gas status)

characteristic ionic charge = +

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

what are group-2 elements

A

alkaline earth metals

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

what do the alkaline earth metals have in common and what is there characteristic ionic charge

A

They all have two electrons in their outer shell or they would like to lose two
electrons to have 8 electrons in their outer shell (achieve Noble Gas status)

characteristic ionic charge = 2+

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

group 3 characteristic ionic charge

A

characteristic ionic charge = 3+

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

group 4 characteristic ionic charge

A

Warning: C 4- or C 4+ both do not exist because the carbon nuclei cannot hold this
larger charge

18
Q

group 5 elements

A

The most important one is N
It has 5 electrons in its outer shell and would like 3 electrons to complete the
Octet, hence its most characteristic ionic charge is

19
Q

Group 6-Elements S and O what do they both have in common

A

Oxygen and Sulphur both have 6 electrons in their valence shells, therefore they would like to gain two electrons to complete the octet and achieve their Noble gas electronic structure.

20
Q

Group 6-Elements S and O What is their characteristic ionic charge?

A

S2- O2-

21
Q

what are the group 7 elements called

A

halogens

22
Q

group 7 elements details lol

A

All have 7 electrons in their valence shells, therefore they would like to gain
one electron to complete the octet and achieve there Noble gas electronic
structure.

23
Q

group 7 elements characteristic ionic charge

A

F -, Br -, Cl -,

24
Q

what is the ion nomenclature for cations and give two examples

A

just the elements name lol, hydrogen = hydrogen, sodium = sodium

25
Q

what is the ion nomenclature for anions and give two examples

A

suffix -ide, fluorine = fluoride, chlorine = chloride

26
Q

covalent bond definition

A

Results from the force of Attraction
Between Two Atoms in the mutual
Sharing of electrons

27
Q

what is a chemical bond known as

A

an intramolecular force

28
Q

what happens in a covalent bond

A

Electrons are shared between two or more atoms

The two atoms share a pair of electrons (one from each atom) and it fills the valence shell of each atom

29
Q

how can a covalent bond form

A

Can form between: two non-metals or a non-metal and a metalloid

Covalent bonds results when electrons are shared by nuclei.

30
Q

what is the mutual sharing of 2 electrons

A

a single bond

31
Q

what is the mutual sharing of 4 electrons

A

a double bond

32
Q

what is the mutual sharing of 2 electrons

A

a triple bond

33
Q

what is a quadruple bond

A

non-existant

34
Q

Electronegativity definition

A

The relative ability of a bonded atom to attract shared electron
s

35
Q

what is a pure covalent bond

A

A “pure” covalent bond would be a bond in which the pair of electrons
is shared equally between the two bonded atoms. e.g. H-H

36
Q

In an ionic bond the pair of electrons resides where ?

A

In an ionic bond the pair of electrons resides completely on the more
electronegative atom

37
Q

what are non-bonding electron pairs called

A

lone pairs

38
Q

difference in electronegativity between bonded atoms for polar covalent bonds

A

0.5 to 1.9

39
Q

difference in electronegativity between bonded atoms for non-polar covalent bonds

A

less than 0.5

40
Q

difference in electronegativity between bonded atoms for ionic bonds

A

greater than 1.9

41
Q

electronegativity trends in the periodic table

A

Increases up the group, because of the decreasing distances of the
outer shell electrons from the nucleus

Increases to the right because of the increasing positive charge of the nucleus

Elements which have low electronegativites are considered electropositive

42
Q

what does the polarity of a bond depend on

A

The polarity of a bond depends on the difference between the electronegativity
values of the atoms forming the bond.

43
Q
A

Introductory Chemistry Flashcards (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions