Brainscape's Knowledge GenomeTM

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


See full index

Physical chemistry > Bonding > Flashcards

Bonding Flashcards

1
Q

Give the diagram (arrow) that shows how structure relates to bonding and bonding relates to structure

A

Check physical flashcards to see if you got it right

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

What is a chemical bond?

A

An attractive force holding together two or more atoms, molecules or ions

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

When atoms bond, what are they trying to form?

A

A noble gas configuration

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

How do elements achieve a noble gas configuration?

A

By sharing, loosing or gaining electrons

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

List the types of bonding

A
  • Covalent bonding
  • Ionic bonding
  • Metallic bonding
  • Dative covalent bonding
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What are the two types of covalent bonding?

A

Simple molecular covalent bonding and giant molecular covalent bonding

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

What is bonded in an ionic bond?

A

Metals and Non-metals

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

What is bonded in covalent (molecular) bonding?

A

Two non-metals

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

What is bonded in metallic bonding?

A

Metals

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

Describe the bonding in ionic compounds

A

Ionic bonding between oppositely charged IONS
Bonding between metals ( positive charge) and non metals (negative charge)

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

Give examples of ionic compounds

A

NaCl and K2CO3

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

What is the structure of ionic bonds?

A

Giant ionic lattice

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

List the properties of ionic bonds? (6)

A
  • High melting point
  • Don’t conduct electricity when solid due to rigidity of IONS so they cant move
  • however, they conduct electricity when molten (liquid) because IONS are free to move so they can conduct electricity
  • The higher the charge, the stronger the ionic bond
  • The smaller the ion, the stronger the ionic bond
    They require lots of energy to overcome the force of attraction
  • Strong electrostatic forces of attraction between oppositely charged ions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are you NOT expected to talk about when describing ionic bonds

A
  • Metallic bonds
  • Electronegativity
  • Dipoles
  • Electrons moving
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

List four factors that determine stronger ionic bonds

A

• Smaller ionic radius
Greater ionic charge, the greater charge density
• Stronger electrostatic forces of attraction between oppositely charged ions
• more exothermic (more negative) lattice enthalpy

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

Give another type of crystal structure

A

Metals

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

Describe the bonding between metals

A

Metallic bonding due to attraction between positively charged metal ions and a ‘sea’ of de localized electrons

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

What is the structure of metals?

A

Giant metallic lattice

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

What determines the strength of a metallic bond

A

•The higher the positive charge on the metal ion, the stronger the metallic bond
• Smaller the ion the higher the charge density and the stronger the metallic bond

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

Give the properties of metals

A

• High melting point
• Conduct electricity when solid
• When molten (liquid) they are good heat conductors
• Higher the charge on the ions, the stronger the bonds

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

Give the reasons for the properties in metals

A

• Strong electrostatic forces of attraction between positively charged metal ions and a sea of delocalized electrons

• A sea of delocalized electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Why can metals be beaten to different shapes?

A

They are are malleable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Give reasons for why metals are malleable

A

Layers of atoms can fairly easily slide over each other without breaking the bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

List the types of intermolecular forces

A

• Permanent dipole dipole interaction
• Vanderwaals forces of attraction
• Hydrogen bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What are the elements that form hydrogen bonds

A

• N-H
• O-H
• F-H

26
Q

What is the bond angle in water?

A

104.5

27
Q

Which of the intermolecular forces is the weakest?

A

Vander waals

28
Q

What is simple molecular covalent bonding?

A

Strong covalent bonds between the atoms, weak vander waals forces of attraction between the molecules

29
Q

Are there any lone electrons in simple covalent bonding?

A

No - all involved in bonding

30
Q

Can simple covalent molecules conduct electricity and why?

A

No all electrons used in bonding so they are not free to move

31
Q

Do simple covalent molecular substances have a high/low mpt and bpt? Why?

A

Low- weak vander waals forces of attraction between molecules that do not require much energy to break

32
Q

Describe macro molecular covalent bonding

A

Lattice in many atoms held together by strong covalent bonds

33
Q

Do macromolecular substances have high mpt and bpt?

A

Yes - lots of energy required to overcome strong covalent bonds

34
Q

Define electronegativity

A

The ability of an atom to attract a pair of electrons in a covalent bond

35
Q

What affects electronegativity?

A

• Nuclear charge
• Atomic radius
• Electron shielding

36
Q

What is the most electronegative element?

A

Fluorine, 4.0

37
Q

How do you get a non polar bond

A

When bonding elements have the same electronegativity

38
Q

What is the strongest intermolecular force?

A

Hydrogen bonding

39
Q

How do you have a polar bond but not a polar molecule?

A

Different electronegativity but symmetrical

40
Q

Describe vander waals forces of attraction

A

• Temporary dipoles created by random movement of electrons
• Induced dipole in neighboring molecule
• Temporary induced dipole attraction

41
Q

Which molecules are vander waals forces stronger?

A

Larger molecules

42
Q

Describe permanent dipole-dipole attraction

A

• Difference in electronegativity of elements
• Vander waals forces between molecules
• Covalent bonds between elements

43
Q

Draw a molecule of water

A

Check physical flash cards to see if you got it right

44
Q

Why is ice less dense that water?

A

• In liquid hydrogen bonds are constantly breaking and reforming as molecules move about
• In ice hydrogen bonds hold the molecules in a fixed position. This makes them slightly further apart in liquid water

45
Q

What is a dative covalent bond/Coordinate bond? And when is it formed?

A

Formed when an electron deficient atom/ion accepts a lone pair of electrons from an atom/ion with a lone pair of electrons (not used in bonding). A covalent bond in which both electrons come from the same atom

46
Q

Draw the forming of a dative covalent bond in ammonia

A

Check physical flash cards to see if you got it right

47
Q

Note

A

• Always draw out the shape when answering questions
• Covalent is sharing
• Take not of Dative/coordinate bonds
• Electrostatic
• Iodide is a bigger ion so it will have less attraction to Sodium ion

48
Q

How can we determine the shape of a molecule

A

• Number of electrons in valence shell of atom
• Number of bonded electrons
• Total of all electrons
• Divide by number of atoms
• Number of bonded atoms
• Subtract to get lone pairs
• Shape
• Angle

49
Q

What does the electron pair repulsion theory state?

A

• Electron pair will take up positions as far away from each other as possible, to minimize the repulsive forces between them

50
Q

What is the order of electron repulsion in a substance

A

• LP-LP
• LP-BP
• BP- BP

51
Q

List types of shapes and their angles

A

• Linear = 180*
• Tetrahedral = 109.5*
• Trigonal bipyramidal = 120/90
• Trigonal planar = 120*
• Octahedral = 90*
• Bent/v-shaped = 104.5*
Square planar= 90*

52
Q

Note

A

• Read the flipping question
• Pair of electrons on - donate to -
• Strong
• To explain the shape of a molecule: Discuss pair repulsion theory and balancing of bonds attached e.g electron pairs equally repel each other
• BETWEEN THE MOLECULES
• Bigger not larger
• Be careful when deducing a similar shape

53
Q

Structure of graphite

A

• Vander waals forces between the molecules
• strong covalent bonds within the layers
• Layers of carbon atoms
• Lots of energy required to break many covalent bonds

54
Q

Which intermolecular force is the highest?

A

hydrogen bonding

55
Q

Describe vander waals forces of attraction

A
  • Similar electronegativity
    -symmetrical molecules
    -Intermolecular force
56
Q

Every molecule/ compound has what?

A

Vander waals forces of attraction

57
Q

Describe metallic bonding

A

• Strong electrostatic force of attraction between positively charged metal ions and a sea of delocalised electrons
• High melting point
• metallic lattice structure
• Conduct electricity when solid
• Conduct electricity when molten

58
Q

Describe permanent dipole-dipole interaction bonding

A

• Strong covalent bonds between the atoms with different electronegativities
• Slight positive and negative charges attract opposite adjacent molecules
• Don’t conduct electricity
• More soluble in water
• Polarised
• Melting points are low but relatively higher than non-polar molecules

59
Q

Which is a smaller ion, Mg2+ or Na+ and why and which will form a stronger ionic bond

A

• Mg2+ is a smaller ion than Na+ (ionic radius)
• Mg2+ has a higher charge density because 2+ is in a much smaller volume
• Mg2+ will form stronger ionic bonds

60
Q

What is the most likely bond angle around the oxygen atom in ethanol and why?

A
  • 104.5
  • It is bonded to hydrogen and carbon which means it has two lone pairs left making the bond a bent/v-shape
61
Q

hydrogen bonding is found where?

A

between the molecules

Physical chemistry (10 decks)

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