Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Bonding > Flashcards

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 type of bonding exists between metals and non-metals

A

Ionic bonding

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

What happens to electrons in ionic bonding

A

They are transferred from metal to non-metal

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

Describe the nature of an ionic bond

A

The electrostatic attraction between oppositely charged ions

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

Describe the structure of ionic compounds

A

Giant ionic lattice of positive and negative ions held together by electrostatic forces

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

Explain the melting point of ionic compounds

A

High melting point because strong electrostatic forces within ionic lattice which require a great deal of energy to break

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

Explain the electrical conductivity of ionic compounds

A

Conduct when molten or dissolved because ions can move but do not conduct as a solid because ions held in fixed position in lattice

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

Which would you expect to have a higher melting point, NaCl or MgO and why

A

MgO because ions are double the charge of NaCl so stronger electrostatic forces

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

What is the formula of the ionic compound Aluminium Sulfate

A

Al2(SO4)3

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

What happens to electrons in covalent bonding

A

Electrons are shared between non-metal atoms

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

What is the difference between a single and double covalent bond

A

Single is 2 shared electrons in bond, double is 4 shared electrons

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

Describe the bonding in diamond

A

Each carbon is bonded to 4 other carbons in a tetrahedral shape

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

Describe the structure of graphite

A

Layers of carbon atoms arranged in hexagonal pattern with weak bonds and delocalised electrons between layers

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

Explain why graphite conducts electricity

A

Delocalised electrons are free to move and carry charge

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

Explain the hardness of diamond

A

Atoms are held in fixed positions

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

What is a co-ordinate (dative) bond

A

Where one atom contributes both electrons in a covalent bond

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

Give an example of a molecule with co-ordinate bonding

A

NH4+, AlCl3NH3, CO

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

Why do molecules have different shapes?

A

Electron pairs repel each other as far apart as possible.

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

Which has the greater repulsion effect lone pair of electrons or a covalent bond?

A

Lone pair

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

What is the bond angle in a linear molecule?

A

180°

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

What is the bond angle in a trigonal planer molecule?

A

120°

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

What is the bond angle in a tetrahedral molecule ?

A

109.5°

22
Q

What shape molecule has 6 bonding electron pairs eg SF6, and what is the bond angle

A

Octahedral, 90 degrees

23
Q

What shape molecule has 5 bonding pairs eg. PCl5 and what are the bond angles

A

Trigonal bipyramidal, 90 degrees and 120 degrees

24
Q

What is the shape and bond angle of CH4. Why

A

Tetrahedral, 109.5 degree, electron pairs repel each other as far as possible

25
Q

How do lone pairs affect bond angles

A

Reduce bonding pair bond angles (by approx. 2 degrees per lone pair) as they repel more than bonding pairs

26
Q

What is the shape and bond angle in water. Why

A

Bent, 104.5 degree, 4 pairs of electrons including 2 lone pairs

27
Q

What is the shape and bond angle in ammonia. Why

A

Trigonal Pyramidal, 107. degree, 4 pairs of electrons including 1 lone pair

28
Q

What is the shape and bond angle in SiCl62- Why

A

Octahedral, 90. degree, 6 bonding pairs of electrons 0 lone pairs

29
Q

Why is the is the bond angle in water less than 180°?

A

Water contains two bonds and two lone pairs. Lone pairs repel further than bonded pairs of electrons.

30
Q

Where in the periodic table are the most electronegative elements

A

Top right (not including noble gases)

31
Q

Which is the most electronegative element

A

Fluorine

32
Q

Which of these bonds will have a dipole? H-C or Cl-C

A

Cl-C

33
Q

What causes molecule to be polar (2 requirements)

A

significant differences in electronegativity and asymmetrical shape

34
Q

Why is CCl₄ not a polar molecule?

A

Symmetrical molecule so dipoles cancel out.

35
Q

Define electronegativity

A

The ability of an atom to attract electron density (the electron pair) in a covalent bond

36
Q

What causes bond polarity

A

Differences in electronegativity between two atoms bonded together

37
Q

Name the 3 types of intermolecular force in order from weakest to strongest

A

Van der Waals, dipole-dipole and hydrogen bonding

38
Q

Which type of intermolecular force exists between diatomic molecules

A

Van der waals only

39
Q

Which types of intermolecular force exist in carbon dioxide

A

Dipole dipole forces

40
Q

Explain how Van der Waals forces arise

A

Temporary dipoles because of movement of electrons which induce temporary dipoles in neighbouring molecules

41
Q

Explain how dipole dipole forces arise

A

Partial positive charge attracting partial negative charge

42
Q

Explain why the boiling point of alkanes increase with increasing chain length

A

More Van der Waals forces

43
Q

Describe the structure of iodine

A

Molecular lattice of I2 molecules held tougher by Van der Waals forces

44
Q

What 3 elements could be bonded to hydrogen to give hydrogen bonding

A

Oxygen, nitrogen or fluorine

45
Q

What is a hydrogen bond?

A

an electrostatic attraction between a proton in one molecule and an electronegative atom in the other.

46
Q

How does hydrogen bonding affect boiling point

A

Increases boiling point

47
Q

Describe the structure of ice

A

Regular lattice structure of water molecules held together by hydrogen bonding. Less dense than water

48
Q

Describe the strucutre of metals

A

Giant metallic lattice of positive metal ions surrounded by delocalised electrons

49
Q

Explain why Mg has a higher melting point than Na

A

Doubly charged metal ion

50
Q

Explain why metals conduct electricity

A

Delocalised electrons are free to move and carry charge

51
Q

Explain why metals have high melting points

A

The delocalised electrons are strongly attracted to the positive metal ions (strong metallic bonds) which requires a lot of energy to overcome

Chemistry (21 decks)

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