Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Structure + Bonding > Flashcards

Structure + Bonding Flashcards

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

what is an atom?

A

the smallest part of an element that can exist, composed of protons, neutrons and electrons

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

what is an element?

A

a substance that only contains one type of atom

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

what is a compound?

A

contains 2 or more elements which are chemically combined in fixed proportions held together by chemical bonds

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

how are elements separated in compounds?

A

by electrolysis or chemical reactions

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

what are reactants?

A

the substances that react. usually on the left side of an equation

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

what are products?

A

the new substances that are formed. usually on the right side of an equation

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

what are mixtures?

A

consist of two or more elements or compounds which are not chemically bonded together

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

what is filtration?

A

used to separate soluble solids from insoluble solids

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

what is crystallisation?

A

used to obtain a soluble solid from a solution, such as salt from salt water

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

what is simple distillation?

A

technique used to separate a substance from a mixture due to a difference in boiling points of the components in a mixture

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

what is the relative mass of protons and neutrons?

A

1

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

what is the relative mass of an electron?

A

0

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

what charge does proton have?

A

+1 or positive

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

what charge does a neutron have?

A

0

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

what charge does an electron have?

A

-1 or negative

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

whats the radius of an atom?

A

0.1nm or 1 x 10^-10m

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

what is the relationship between the number of protons and electrons?

A

they are equal so they cancel out, making the atom neutral

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

what is an ion?

A

when the atom loses or gains electrons, making it charged

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

what makes an ion negative?

A

when there is more electrons than protons (non metals)

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

what makes an ion positive?

A

when there is more protons than electrons (metals)

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

what is an elemental symbol?

A

the one or two letter symbol that represents the element in a periodic table

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

what does the atomic number tell us? (bottom left number)

A

the number of protons and electrons the element has

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

what does the mass number tell us? (top left number)

A

total number of protons and neutrons in that atom

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

whats the radius of the nucleus of an atom?

A

1 x 10^-14

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

how would you calculate the number of neutrons in an atom?

A

mass number subtract atomic number

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

what determines an element?

A

the number of protons determines what type of atom it is. for example, 1 proton makes hydrogen

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

what is an isotope?

A

same number of protons but a different number of neutrons so they have the same atomic number but different mass numbers

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

how do you calculate relative atomic mass?

A

relative atomic mass = (the sum of isotope abundance and isotope mass number) / sum of abundance of all isotopes

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

what is relative atomic mass?

A

as many elements can exist as a number of different isotopes, relative atomic mass is used instead of mass number when referring to the element as a whole. this is an average mass taking into account the different masses and abundance (amount) of all isotopes

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

what is ionic bonding?

A

a compound made up of metal and non metal consists of ions. the metal atoms lose electrons to form positive ions and the non metal atoms gain electrons to form negative ions. the opposite charges mean that they are strongly attracted to each other and have strong electrostatic forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

what is covalent bonding?

A

a compound formed from non metals consists of molecules which each share electrons with other atoms, the positively charged nuclei of the bonded atoms are attracted to the shared pair of e- by electrostatic forces making covalent bonds very strong

32
Q

what is the formula for carbon dioxide?

A

CO2

33
Q

what is the formula for ammonia?

A

NH3

34
Q

what is the formula for water?

A

H2O

35
Q

what is the formula for sodium chloride?

A

NaCl

36
Q

what is the formula for carbon monoxide?

A

CO

37
Q

what is the formula for hydrochloric acid?

A

HCl

38
Q

what is the formula for calcium chloride?

A

CaCl2

39
Q

what is the formula for sodium carbonate?

A

Na2CO3

40
Q

what is the formula for sulfuric acid?

A

H2SO4

41
Q

what makes elements stable?

A

full outer shell of electrons

42
Q

what is the structure of ionic compounds?

A

giant ionic lattice structure where positive and negative ions alternate, meaning they are attracted to all those around it. regular lattice with strong electrostatic forces

43
Q

what are properties of ionic compounds?

A

high boiling and melting points as they have very strong electrostatic bonds so require loads of energy to break. they also conduct electricity when they are molten or aqueous as ions or delocalised electrons are free to move and can carry a charge (ions can flow to oppositely charged electrodes)

44
Q

whats the formula for a hydroxide ion?

A

OH-

45
Q

what is the formula for a sulfate ion?

A

SO4 2-

46
Q

what is the formula for a nitrate ion?

A

NO3-

47
Q

what is the formula for a carbonate ion?

A

CO3 2-

48
Q

what is the formula for a ammonia ion?

A

NH4+

49
Q

what is a disadvantage of displayed formula?

A

it does not show 3D structure or which atoms the e- in the covalent bond have come from

50
Q

what is a disadvantage of 3D models?

A

it is hard to predict what shape the molecule will make, and only allows us to see the outer layer of a compound

51
Q

what are the properties of simple molecular substances made with covalent bonds?

A

small molecules in which the atoms are joined together (as they share e-) by strong covalent bonds but between the molecules there is weak intermolecular forces which can easily break, meaning low melting/boiling points. for example, H2O and CH4

52
Q

what is the formula for methane?

A

CH4

53
Q

what other 2 substances are made from covalent bonds?

A

polymers and giant covalent structures

54
Q

can simple covalent substances conduct electricity?

A

no, as they contain no charged particles

55
Q

what are the properties of giant covalent structures?

A

carbon and silicon dioxide form a giant covalent lattice which has lots of strong covalent bonds which are hard to break so have a high melting point.

56
Q

what are examples of giant covalent structure in terms of carbon?

A

carbon makes diamond (4 bonds), graphite, graphene and carbon nanotubes (all 3 bonds). in silicon dioxide, each silicon atom is bonded to 4 oxygen atoms and each oxygen atom to 2 silicon

57
Q

what are properties of metallic substances?

A

form a giant metallic lattice and each metal atom releases its outer most electrons from its structure meaning they all form positive ions in a sea of delocalised electrons. they allows metals to be good conductors as the electrons can move and flow. they also have a high melting point due to strong electrostatic forces

58
Q

why are metals malleable?

A

ions are arranged in layers that can slide over each other

59
Q

what groups likely form ions?

A

1,2,6,7

60
Q

what type of ions are group 1 and 2?

A

they are metals so lose e- to form positive ions called cations

61
Q

what type of ions are group 6 and 7?

A

they are non metals so gain e- to form negative called anions

62
Q

what charge do group 1 ions have?

A

1+

63
Q

what charge do group 2 ions have?

A

2+

64
Q

what charge do group 6 ions have?

A

2-

65
Q

what charge do group 7 ions have?

A

1-

66
Q

what are disadvantages of a ball and stick diagram?

A

in reality, there is no gaps between ions

67
Q

what are the disadvantages of a cross and dot diagram?

A

do not show the relative sizes of the atoms or how the atoms are arranged in space

68
Q

what is a polymer?

A

long chains of repeating units/small units are linked together to form a long molecule

69
Q

what bonds make up polymers?

A

strong covalent but the intermolecular forces between polymer molecules is larger than simple covalent substances so they need more energy to overcome

70
Q

do giant covalent structures conduct electricity?

A

no as they do not contain charged particles

71
Q

what is the structure of diamond?

A

giant covalent structure make up of carbon atoms that each form 4 covalent bonds. this makes diamond hard as the strong bonds take lots of energy to break which gives a high melting point.

72
Q

can diamond conduct electricity?

A

no as it has no free e- or ions

73
Q

what is the structure of graphite?

A

made up of carbon atom that forms 3 covalent bonds creating sheets of carbon atoms arranged in hexagons, they have a high melting point so require loads of energy to break.

74
Q

why does graphite make a good lubricant?

A

there are not covalent bonds between layers, theyre held together weakly so free to slide over each other making it soft and good for lubricant

75
Q

can graphite conduct electricity?

A

only 3 out of 4 e- are used in bonds so each carbon atom has a free e- which can conduct

76
Q

what is the structure of graphene?

A

graphene is only one sheet of graphite so carbon atoms joined in hexagons. its one atom thick making it 2D. the network of covalent bonds is very strong but also very light so can be added to composite materials without affecting the weight

77
Q

can graphene conduct electricity?

A

yes as it contains delocalised e- which can move throughout the whole structure so can be used in electronics

Chemistry (3 decks)

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