Brainscape's Knowledge GenomeTM

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


See full index

Chemistry Content > Bonding > Flashcards

Bonding Flashcards

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

Metallic bonding

A
  • GML
  • positive ions in a regular lattice
  • delocalised electrons
  • stronger metallic bonding when
    • smaller ion
    • more charge on the ions
    • higher forces of electrostatic charge between delocalised electrons and positive ions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Properties of metals

A
  • good conductors of heat and electricity
  • strong
  • malleable and ductile
  • high melting point
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Why are metals good conductors

A
  • delocalised electrons are able to move freely thronging the structure
  • ions are closely packed and so pass vibrational energy on more effectively
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are metals malleable and ductile

A
  • the layers OF ATOMS slide over each other
  • malleable - beat into shape
  • ductile - drawn into thin wires
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Ionic bonding

A
  • GIL
  • one loses electron and one gains an electron creating ions.
  • metals are cations, non-metals are anions
  • the smaller the ions and the greater charge of the ions, means many strong forces of attraction between positive and negative ions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Properties of ionic compounds

A
  • GIL
  • High melting point
    • many strong forces of attraction b/w positive and negative ions
  • conductivity
    • when dissolved in water or molten, ionic compounds conduct electricity so that ions can move and conduct electricity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Ammonium

A

NH4+

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

Nitrate

A

NO3-

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

Mercury

A

Hg2(2+)

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

Cyanide

A

CN-

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

Hydroxide

A

OH-

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

Peroxide

A

O2(2-)

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

Sulphate

A

SO4(2-)

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

Carbonate

A

CO3(2-)

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

Phosphate

A

PO4(3-)

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

Permanganate

A

MnO4-

17
Q

Dichromate

A

Cr2O7(2-)

18
Q

Acetate

A

C2H3O2-

19
Q

Dative covalent bonding

A

Is a covalent bond in which both electrons come from the same atom
It is drawn with an arrow rather than a —

20
Q

Covalent bonding

A
  • SCM

- GCL

21
Q

Potassium vs aluminium

A

Aluminium

- smaller ion as less shells 
- higher charge
- stronger forces of attraction b/w ion and delocalised electrons
22
Q

Order of repulsive powers with shapes of molecules

A
  1. Lp-lp
  2. Lp-bp
  3. Bp-bp

Lp-bp has a greater repulsion than bp-bp

23
Q

Degree of linear shape

A

180

24
Q

Degree of trigonal planar

A

120

25
Q

Degree of tetrahedral

A

109.5

26
Q

Degree of trigonal bipyramid

A

120, 90

27
Q

Degree of octahedral

A

90

28
Q

Summary of shapes of molecules

A
29
Q

Electronegativity

A

This is the measure of the tendency of an atom to attract a bonding pair of electron in a covalent bond

30
Q

What determines electronegativity

A
  1. Nuclear charge
    - more protons
    - stronger attraction between nucleus and BONDING PAIR of electrons
  2. Atomic radius
    - closer to the nucleus
    - stronger attraction between nucleus and bonding pair of electrons
  3. Shielding
    - less shells of electrons between the nucleus and electrons
    - less shielding
    - stronger attraction between nucleus and bonding pair of electrons
31
Q

Trend of electronegativity in a period

A
  • increases
  • all electrons are the same distance from nucleus
  • proton number increasing
  • atoms are getting smaller
  • shielding is the same
  • so stronger attraction between nucleus and 2 electrons in covalent bond
32
Q

Electronegativity down a group

A
  • decreases
  • increase atomic radius
  • electrons are further away
  • more shells/ more shielding
  • reduced force of attraction between nucleus and 2 electrons in covalent bond
33
Q

Polar bond

A
  • one of the atoms holds the electrons closer to itself in the bond
  • one end of the bond will be slightly negative due to the electrons being there
  • the other end will be slightly positive due to the electrons not being there
34
Q

Diff types if imf

A

Hydrogen
Dipole-Dipole
VDW

35
Q

Which bonding type do you only mention imf

A

SCM

Inter MOLECULAR forces - simple covalent MOLECULES

36
Q

Noble gas boiling points down group

A
  • increases
  • more shells
  • more shielding
  • more electrons, so more vdw forces
37
Q

Different types of crystal structures

A
  • GIL
  • GML
  • Macromolecular (GCM)
  • Molecular (SCM)

Chemistry Content (31 decks)

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