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Chemistry > C2b - Bonding > Flashcards

C2b - Bonding Flashcards

1
Q

1 appearance of metal
non-metal

A

metal- shiny
NM- dull

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2
Q

1 melting point and boiling point
metal and NM

A

metal- high
NM- low

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3
Q

1 state at room temperature
M and NM

A

M-solid
NM-half are solid, half are gas

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4
Q

1 malleable or brittle
M or NM

A

M- malleable
NM-brittle

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5
Q

1 what does malleable mean

A

bend without shattering

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6
Q

1 what does brittle mean

A

shatter when hammered

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7
Q

1 ductile or not
M and NM

A

M- ductile
NM- non-ductile

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8
Q

1 what does ductile mean

A

can be pulled into wires

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9
Q

1 thermal and electrical conductors
M and NM

A

M- good conductor
NM- poor conductor (insulator)

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10
Q

1 low or high density
M and NM

A

M- high
NM- low

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11
Q

1 sonorous or dull
M and NM

A

M- Sonorous
NM- dull

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12
Q

1 what does sonorous mean

A

makes a ringing sound when hit

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13
Q

1 where are metals on the periodic table
example?

A

left and middle
Cu- Copper

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14
Q

1 where are the non-metals
example

A

diagonal corner on the right
except hydrogen on the top left
H- hydrogen

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15
Q

1 what is in between the metals and non-metals

A

metalloids

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16
Q

1 name the 7 metalloids

A

boron
silicon
germanium
arsenic
tellurium
polonium
antinomy

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17
Q

1 what is a metalloid

A

contains properties from metals and non-metals

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18
Q

1 what is a chemical property

A

a characteristic of a substance that can only be observed through chemical reactions

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19
Q

1 chemical properties of metals

A

lose electrons to form positive ions
don’t react with each other

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20
Q

1 chemical properties of non-metals

A

gain electrons to form negative ions
react with each other to produce compounds consisting of molecules

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21
Q

1 chemical properties of metal oxides

A

produce alkaline solutions

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22
Q

1 chemical properties of non-metal oxides

A

produce acidic solutions

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23
Q

2 what is a period

A

a horizontal row

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24
Q

2 what is a group

A

a column

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25
Q

2 how is the periodic table arranged

A

goes up in atomic number (electrons increase each element)
element in a group have similar chemical properties

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26
Q

2 how are electrons arranged in atoms

A

in the first shell is 2 electrons
the second is 8
the third is 8
the fourth is 2 - up to the 20th element

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27
Q

2 how does electronic structure help the periodic table

A

the last number equals amount of electrons in the outer shell
the number of number is the period
the sum of the numbers equals the atomic number

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28
Q

1 what si the electronic structure of oxygen (8)

A

2.6

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29
Q

1 what si the electronic structure of silicon (14)

A

2.8.4

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30
Q

1 what si the electronic structure of calcium (20)

A

2.8.8.2

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31
Q

2 charge of an atom?

A

no overall charge
positively charged protons = negatively charged electrons
no. of electrons = atomic number

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32
Q

3 what is an ion

A

an electrically charged particle formed when an atom loses or gains electrons
metals lose electrons to become +ive
non-metals gain electrons to become -ive
no. of protons and neutrons does not change

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33
Q

3 how does Na become Na+

A

loses an outer electron

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34
Q

3 how does Mg become Mg2+

A

loses two outer shell electrons

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35
Q

3 how does Cl become Cl-

A

gains an outer shell electron

36
Q

3 how does O become O2-

A

gains two outer shell electrons

37
Q

3 what are electronic structures of ions

A

Sodium is 2.8.1
loses one electron
is now 2.8

38
Q

3 what are electron diagrams

A

represents the shells of an ion or atom
draw with crosses or dots as electrons
charge is written at top right

39
Q

4 how do ionic compounds form

A

when a metal reacts with non-metal
electrons transfer
metal becomes +ive cations
non-metal becomes -ive anions

40
Q

4 how do sodium and chlorine react with each other

A

Na - 2.8.1
Cl - 2.8.7
sodium gives away an electron so they both achieve full outer shells

41
Q

4 what is structure and bonding in ionic compounds

A

solid state, arranged regularly- giant ionic lattice
ions held in by ionic bonds

42
Q

4 what are ionic bonds

A

strong electrostatic forces or attraction between oppositely charged ions

43
Q

4 what does giant ionic lattice mean

A

repeated many times
contains ions
arranged regularly

44
Q

4 what is bonded when its an ionic bond?

A

a metal and a non-metal

45
Q

5 what are covalent bonds

A

a shared pair of electrons
two non-metal atoms share an electron in their outer shells

46
Q

5 how do you show covalent bonds on a dot and cross diagram

A

overlap the circles like a venn diagram
add the two electron into that bit instead of drawing them on the lines

47
Q

5 what are simple molecules

A

hydrogen, oxygen, water and carbon dioxide
non-metal atoms are joined together by covalent bonds
only contains a few atoms
all be modelled using a dot and cross diagram

48
Q

5 what are hydrogen, oxygen, water and carbon dioxide formulas

A

hydrogen - H2
oxygen - O2
water - H2O
carbon dioxide - CO2

49
Q

5 what is the structure and bonding in a simple molecule

A

electrostatic forces of attraction
forces between the nucleus and shared electrons
covalent bonds are strong
intermolecular forces are weak

50
Q

5 do simple molecules have high or low melting and boiling points

A

relatively low
strong covalent bonds dont break apart
weak attractive forces between molecules break
called intermolecular forces

51
Q

5 do simple molecules conduct electricity

A

no
there are no free moving electron to carry the current

52
Q

5 pros and cons of molecular formula
ie. CH4

A

pros
-number of atoms of the element
-easy to write

cons
-not 3D
-doesnt show structure or bonding

53
Q

5 pros and cons of displayed formula with bonds
ie O-C-O (CO2)

A

pros
-shows bonding

cons
-not 3D
-gets crowded

54
Q

5 pros and cons of ball and stick model

A

pros
-3D arrangement of atoms

cons
-no physical bonds
-needs colour to identify atoms
-too far apart to be accurate

55
Q

5 pros and cons of space filling models

A

pros
-most realistic
-3D, good accuracy

cons
-bonding is hard to distinguish
-needs colour key

56
Q

6 what is a giant covalent structure

A

many non-metal atoms joined by covalent bonds and arranged in a regular repeating pattern called a giant lattice
also called giant covalent lattices

57
Q

6 why is diamond a giant covalent structure

A

a form of carbon
exist as a giant covalent structure
each carbon atom is joined to 4 other carbon atoms by covalent bond

58
Q

6 what is the formulae of giant molecules

A

similar to ionic, all atoms involved
don’t try and write formula, its too big
you use empirical formula
shows the simplest whole number ratio of atoms
diamond is known as C

59
Q

6 What is the formula for silica

A

each silica is bonded to 4 oxygens
each oxygen bonded to 2 silicon
on average, it is SiO(2)

60
Q

7 what are polymers

A

made from smaller monomers
monomers join end to end in chemical reactions producing polymers

61
Q

7 what is an example of a polymer

A

ethene monomers join to make polyethene (polythene)
amino acids join together to make proteins, like keratin

62
Q

7 how do you show polymers

A

monomers are simple molecules
few non-metals atoms joined by covalent bonds
model by dot and cross diagrams, space fill models and ball and stick models
difficult for polymer molecules

63
Q

7 how do you often see polymers presented

A

drawn in a wavy line
straight lines between them to show covalent bonds
weak intermolecular forces are not shown

64
Q

7 what are polymer sometimes made of

A

different types of monomers
like protein and DNA

65
Q

7 what are most polymers shown as

A

modelled as a repeating unit of monomers
like ethene and polythene

66
Q

8 what is the structure of metals like

A

all solid at room temperature
packed together regularly
form a giant metallic lattice
draw spheres in a regular pattern touching each other

67
Q

8 what are metallic bonds similar to

A

electron leave outer shells of metals forming a sea of electrons around positively charged metal ions
called delocalised electrons

68
Q

8 what are metallic bonds

A

strong electrostatic forces of attraction between delocalised electrons and closely packed metal ions

69
Q

8 what is localised?
what is delocalised

A

localised - restricted to a particular place
delocalised - free to move in its usual place

70
Q

8 what is a model of metallic structure like

A

3D
metallic bonds in all directions
lose some info when presenting structure and bonding

71
Q

9 who was Mendeleev?

A

most successful person to organise the periodic table

72
Q

9 what did Mendeleev use to organise it

A

atomic weights of known elements (relative atomic masses)
knowledge of chemical reactions
knowledge of physical properties

73
Q

9 what was the first organisation like

A

order of increasing atomic weight
grouped similar properties

74
Q

9 what did he swap

A

iodine and tellurium- it suited the chemical properties better
he left spaces for unknown elements and predicted properties of nearby elements

75
Q

9 what was the next attempt Mendeleev did

A

1st table in rows not columns
1871, rotate to be in rows
3 predicted elements discovered in 1875-86

76
Q

9 why is the modern table ordered by atomic number?

A

Mendeleev first organised it without knowing its atomic structure
he died in 1907
1913 henry moseley discovered atomic no. is no. of protons in the nucleus

77
Q

9 what did moseley’s work show

A

seven gaps left to fill in the 1913 table
Mendeleev was right to swap iodine and tellurium

78
Q

10 why was a new group added to the periodic table

A

argon found in 1894
helium found 1895
both are inert gases
neon, krypton, xenon found it 1898
5 gases forming a new group next to group 7

79
Q

10 what is interesting about the patterns of chemical properties

A

elements arranged in order of increasing atomic no.
atomic no. is no. of protons in an atom
no. of electrons = protons
electron structure comes from no. of electrons
electronic structure determines chemical properties

80
Q

10 why are chemical property patterns interesting

A

there is a link between position of elements and chemical properties

81
Q

10 what is the reactivity pattern in group 1,2 and 7

A

group 1 and 2 get more reactive as you go down
group 7 gets less reactive as you go down

82
Q

10 what is the type, reactivity, structure, and ions in

group 1

A

type = metal
reactivity = very reactive
structure = end in 1
ions formed = +1

83
Q

10 what is the type, reactivity, structure, and ions in

group 2

A

type = metal
reactivity = reactive
structure = end in 2
ions formed = +2

84
Q

10 what is the type, reactivity, structure, and ions in

group 7

A

type = non-metal
reactivity = very reactive
structure = end in 7
ions formed = -1

85
Q

10 what is the type, reactivity, structure, and ions in

group 0

A

type = non-metal
reactivity = very unreactive
structure = outer shells are full
ions formed = not reactive

Chemistry (7 decks)

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