Chapter 5 Flashcards

general terms

1
Q

compound

A

a substance that is made up of 2 or more different elements combined together chemically. eg- NaCl

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

molecule

A

a group of atoms joined together. the smallest particle of an element or compound that can exist independently. eg- Cl2

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

octet rule exceptions

A
  1. transition metals
  2. hydrogen, lithium, beryllium tend to achieve 2 electrons in their outer shell rather than 8.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

ion

A

a charged atom or group of atoms

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

ionic bond

A

force of attraction between oppositely charged ions in a compound. always formed between the complete transfer of electrons from one atom to another.

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

charges of ionic compounds

A

g1- 1+
g2- 2+
g3- 3+
g4- 4+ or 4-
g5- 3-
g6- 2-
g7- 1-
g8- no ion

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

7 diatomic molecules

A

hydrogen, nitrogen, fluoride, oxygen, iodine, chloride, bromine

H2, N2, F2, O2, I2, Cl2, Br2

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

transition metals

A

element that forms at least one ion with a partially filled sublevel. properties:
-have variable valency
-widely used as compounds
-usually coloured compounds

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

exceptions to transition metals

A

Sc3+, Zn2+ because they do not have a partially filled d sub-level

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

what forms a single bond

A

when one pair of electrons is being shared between 2 atoms

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

what forms a double bond

A

when two pairs of electrons are shared between 2 atoms

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

what forms a triple bond

A

when three pairs of electrons are shared between 2 atoms

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

what shape are all double and triple bonds

A

linear in shape and single

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

what are the bond energies for single, double, and triple bonds like

A

single- weakest
double- stronger than single
triple- strongest
~ this is due to sigma bonds being stronger than pi bonds

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

sigma bond

A

formed by the head on overlap of 2 orbitals

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

pi bond

A

formed by the sideways overlap of p orbitals

17
Q

how many sigma and pi bonds in each of the 3 bonds

A

single bond- one sigma bond
double bond- one sigma bond and one pi bond
triple bond- one sigma bond and 2 pi bonds

18
Q

properties of ionic bonds

A

-contains a network of ions in the crystal
-usually hand and brittle
-high melting and boiling points
-usually solid at room temp
-conduct electricity when in molten state or when dissolved in water

19
Q

properties of covalent bonds

A

-contain individual molecules
-usually soft
-low melting and boiling points
-usually liquids, gasses or soft solids at room temp
-do not conduct electricity

20
Q

electronegativity

A

the relative attraction that an atom in a molecule has for a shared pair of electrons in a covalent bond

21
Q

uses of electronegativity

A
  1. predict polarity of covalent bonds
  2. predict which compounds are ionic and which are covalent
22
Q

polar covalent bond

A

a bond in which there is an unequal sharing of the pair(s) of electrons. this causes one side to be slightly positive and the other slightly negative.

23
Q

non-polar covalent bond

A

a bond in which there is an equal sharing of electrons

24
Q

electronegativity difference greater than 1.7 means

A

ionic bonding

25
electronegativity difference less and or equal to 1.7 means
covalent bonding
26
electronegativity difference between 0.4 and 1.7 means
polar covalent bond
27
electronegativity difference less than or equal to 0.4 means
non-polar covalent bond
28
exceptions to predicting bonding in compounds
when the shape of the molecule is: 1. linear 2. trigonal planar 3. tetrahedral
29
intramolecular bonding
bonding that takes place within a molecule, i.e. holds the atoms together, i.e. ionic and covalent bonding
30
intermolecular forces
the forces of attraction that exist between molecules, i.e. Van Der Waals forces, dipole-dipole forces, hydrogen bonding
31
Van Der Waals forces
weak attractive forces between molecules resulting from the formation of temporary dipoles (temporary attraction as a result of a shift of electrons) ~ only force of attraction between non-polar molecules ~boiling point increases with atomic mass ~weakest intermolecular bonding
32
dipole-dipole forces
forces of attraction between the negative pole of one polar molecule and the positive pole of another polar molecule. a permanent dipole if formed between 2 polar molecules ~medium strength, therefore average boiling point ~higher boiling point than Van der Waals
33
hydrogen bonds
types of dipole-dipole attraction between molecules in which hydrogen atoms are bonded to nitrogen, oxygen or fluorine.
34
boiling points
affected by intermolecular bonding and molecular mass. if same intermolecular bonding, the larger molecular mass will have the higher boiling point
35
solubility
affected by intramolecular bonding. like dissolves like. water= polar, oil= non-polar