Brainscape's Knowledge GenomeTM

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


See full index

Chem > Chem - 7/8 (bonding) > Flashcards

Chem - 7/8 (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 s bonding

A

how and why atoms come together to make compounds

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

how many types of bonding are there

A

2

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

what are the two types of bonding

A

ionic and covalent

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

what happens to the electrons in ionic bonding

A

electrons are transferred

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

what are valence electrons

A

the electrons on the very outside of an atom

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

why do the noble gases typically not react

A

they have a full outer shell of valence electrons

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

how many valence electrons do most elements want

A

8

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

how many valence electrons does hydrogen want

A

2

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

how many valence electrons does Helium have

A

2

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

would lithium and fluorine form an ionic compound

A

yes

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

would potassium and helium form an ionic compound

A

no

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

is CO2 ionic

A

no

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

is CaS ionic

A

yes

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

what are 3 properties of ionic compounds

A

most are crystalline solids at room temperature
generally have high melting points
can conduct an electric current when melted or dissolved in water

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

why are ionic compounds typically solids at room temperature with high melting points

A

bc of the orderly arrangement of their ions

each ion is attracted to the ion it is next to so there is less repulsions which results in a stable structure

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

why are ionic solids able to conduct electricity when melted or dissolved in water

A

the ions are free flowing

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

how can you model the valence electrons of metal atoms

A

as a sea of electrons

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

what is an alloy

A

a mixture composed of two or more elements, at least one of which is a metal

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

why are alloys important

A

their properties are often superior those of their component elements

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

is the formation of an alloy a chemical or physical change

A

physical because its a mixture and you can separate it into its components

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

what information does a molecular formula provide

A

how many atoms of each element a substance contains

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

what is a molecule

A

a neutral group of atoms joined together by covalent bonds

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

what is a molecular compound

A

a compound that is composed of molecules

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

what is the difference between ionic and covalent bonds

A

ionic bonding involves the transfer of electrons while covalent bonding involves the sharing of electron

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

Does a molecular formula tell you anything about the structure of a molecule

A

No

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

Does a molecular formula tell you anything about the structure of a molecule

A

No

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What representative units define molecular and ionic compounds

A

MC is molecule

IC is a formula unit

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Compare and contrast melting and boiling points of molecular and ionic compounds

A

MC have lower melting and boiling points

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Compare and contrast the states of matter of molecular and ionic compounds

A

Many MC are gases or liquids at room temperature, while many IC are crystalline solids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What is a single covalent bond

A

A bond formed when two atoms share a pair of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is an unshared pair

A

A pair of valence electrons that is not shared between atoms

31
Q

What is a double covalent bond

A

a bond that involves two shared pairs of electrons

32
Q

What is a triple covalent bond

A

a bond formed by sharing three pairs of electrons

33
Q

What is a resonance structure

A

One of the two of more equally valid electron dot structures that have the same number of electron pairs for a molecule or ion

34
Q

What is the VSEPR theory

A

Electrons want to stay far away from each other, so the shape of the molecule will adjust to honor this

35
Q

What does VSEPR stand for

A

Valence shell electron pair repulsion

36
Q

What is the degree of the tetrahedral angle

A

109.5

37
Q

Do unshared pairs affect the structure of molecules

A

Yes

38
Q

What is electronegativity

A

How much a bonded atom likes electrons

39
Q

What us the most e neg element

A

Fluorine

40
Q

What is the least e neg element

A

Francium

41
Q

What does hydrogen have the same e neg as

A

Carbon

42
Q

For which kind of bonds is polarity important

A

Covalent bonds

43
Q

When do you have non polar bonds

A

Anytime two of the same element are bonded together or when Carbon and hydrogen are bonded

44
Q

When do you have a polar bonds

A

All other bonds that aren’t between two of the same element or carbon and hydrogen

45
Q

How are the electrons shared in non polar bonds

A

Evenly

46
Q

How are electrons shared in polar bonds

A

Unevenly

47
Q

What do you need to know in order to find the polarity of molecules

A

Dot structure
Bond polarity
Shape

48
Q

What do we know about a molecule if it only has nonpolar bonds

A

The whole molecule is nonpolar

49
Q

What is the difference between intra and inter

A

Intra - inside/within

Inter - between

50
Q

Are bonds intramolecular or intermolecular

A

Intramolecular

51
Q

What are the 3 types of intermolecular forces

A

Dispersion, dipole-dipole, and hydrogen bond

52
Q

List the intermolecular forces in order of weakest to strongest

A

Dispersion, dipole-dipole, hydrogen bond

53
Q

Is dispersion force for polar or non polar molecules

A

Non polar

54
Q

Is dipole-dipole force for polar or nonpolar molecules

A

Polar

55
Q

Is hydrogen bond force important for polar or non polar molecules

A

Extreme polar

56
Q

When/why do dispersion forces take place

A

Even in nonpolar molecules, the electrons randomly move around, which can randomly make one side of the molecule more negative than the other, making it temporarily polar. The shift of electrons in one molecule induces the same shift in the molecules around it

57
Q

Why are dispersion forces so weak

A

Because they are temporary

58
Q

What happens in dipole-dipole forces

A

A polar molecule induces the same thing in the molecule next to it

59
Q

Why are dipole dipole forces stronger than dispersion

A

Because they are permanent

60
Q

What do we need to form a hydrogen bond

A

Hydrogen bonded in a molecules to N O or F

61
Q

Why are hydrogen bonds so strong

A

Because it’s an attraction between the very positive part of one molecule and the very negative part of one molecule

62
Q

Why are hydrogen bonds possible

A

Because whenever hydrogen bonds with N O or F, it already has less electrons (and no lone pairs; it’s a ‘naked proton’) and then N O and F are all more electronegative than H so it makes N, O, or F super negative and leaves H super positive

63
Q

when elements are shared unequally, chemists characterize these types of bonds as

A

polar covalent

64
Q

metals typically have (high or low) electronegativity values

A

low

65
Q

what kind of bonds does B2 have

A

nonpolar

66
Q

where are the alkali metals

A

the first column

67
Q

if atom X forms a diatomic molecule with itself, what kind of bond is it

A

Nonpolar covalent

68
Q

where are the alkali earth metals

A

the second column

69
Q

where are the transition metals

A

the middle metals

70
Q

where are the metalloids

A

around the staircase

71
Q

where are the halogens

A

second to last column

72
Q

where are the noble gases

A

last column

73
Q

The bonds between the hydrogen and oxygen atoms in a single water molecule are called what?

A

Polar covalent bonds

74
Q

Why is aluminum better than boron, oxygen, or hydrogen to make wire from

A

It is a metal, so it conducts electricity better because it has free flowing electrons

75
Q

The dot structures of charged molecules have to be in what

A

Brackets with the charge written on the outside!!!

Chem (20 decks)

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