lecture 6 - basic fundamentals of chemistry Flashcards

1
Q

what are the 2 features of a 1s orbital

A

spherical shape and holds two electrons of opposite spin

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

what are the 3 features of a 2s orbital

A

spherical in shape, larger than 1s and have a node

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

what are the two features on a 2p orbital

A

dumbbell in shape and have 3 different arrangements

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

what are the 3 rules regarding assigning electrons to orbitals

A
  1. Lower energy orbitals filled before higher energy orbitals
  2. Pauli Exclusion Principle - orbital can hold two electrons of opposite spin
  3. Hund’s rule - e.g. 3 electrons of one spin will fill one half of all 3 orbitals and then the other 3 electrons will fill the other half, of the opposite spin
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what causes ionic bonding

A

the electrostatic charge interaction, created by one element losing electrons and the other gaining them, between the two oppositely charged ions

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

what causes covalent bonding

A

2 non-metals sharing electrons to gain a full outer shell and be stable

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

are non-polar covalent bonds considered to have symmetrical or unsymmetrical electron distribution and why?

A

symmetrical - electrons are shared equally e.g. Carbon-Carbon bonds

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

are polar covalent bonds considered to have symmetrical or unsymmetrical electron distribution and why?

A

unsymmetrical - electrons are not shared equally due to permanent dipoles created by different electronegativities

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

what is the definition of electronegativity

A

a measure of the tendency of an atom to attract a bonding pair of electrons

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

discuss electronegativity regarding metals and non-metals

A

metals have low electronegativity in order to lose electrons, whereas group 7 have very high electronegativities to gain electrons

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

in regards to electronegativities, when do non-polar covalent bonds form

A

when two atoms have similar or the same electronegativity

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

in regards to electronegativity, when do polar covalent bonds form

A

when two atoms electronegativities differ by 0.3-2.0 arbitrary units

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

in regards to electronegativity, when do ionic bonds form

A

when the difference in electronegativity between two atoms is greater than 2.0 arbitrary units

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

what do functional groups determine

A

the reactivity of a molecule

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

what changes can occur when different functional groups are added to a molecule

A

polarity, the addition/deletion of double bonds, addition/deletion of lone pairs

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

what functional group has the highest priority

A

carboxylic acid

17
Q

what is the order of priority of functional groups

A

carboxylic acid
carbonyl
hydroxy
alkynes
alkenes
alkanes

18
Q

what are terminal and internal alkenes determined by

A

the positions of the double bond

19
Q

Z isomers are?

A

cis - same side

20
Q

E isomers are?

A

trans isomer - opposite

21
Q

what determines a molecule to be an alkyne

A

a carbon-carbon triple bond

22
Q

how do benzene rings work

A

the double bonds have pi electrons which can move between the bonds, creating resonance structures

23
Q

what are the 3 types of Di-substituted benzenes and when do they occur

A

1,2 - Ortho benzene
1,3 - Meta benzene
1,4 - Para benzene

24
Q

what is the difference between a primary, secondary and tertiary alcohol/amine

A

primary - 1 R group
secondary - 2 R groups
tertiary - 3 R groups

25
Q

what do we use to show how many hydrogens have been replaced on an amine

A

an N for each hydrogen

26
Q

what does an amide contain that an amine doesn’t

A

a double bonded oxygen on the same carbon as the nitrogen

27
Q

what do all esters contain

A

O=C-O