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Chem C1-C3 > C2.2 - Bonding > Flashcards

C2.2 - Bonding Flashcards

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1
Q

Describe the properties of metals

A
  • shiny
  • high melting + boiling point
  • malleable
  • ductile (pulled into wires)
  • good conductors
  • solid at room temp
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2
Q

Describe the properties of non-metals, incl what state

A
  • dull
  • low melting + boiling points
  • half are solid, half are gas at room temp
  • brittle
  • non-ductile
  • insulators
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3
Q

What are elements arranged in order of on the periodic table?

A

Atomic number (num. of protons and electrons)

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4
Q

define the periodic table

A

a table in which elements are arranged in columns and periods in ascending order of atomic number

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5
Q

where are metal elements placed in a periodic table?

A

on the left hand side

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6
Q

where are non-metals placed on a period table?

A

on the right hand side

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7
Q

what happens when metals become ions?

do metals react with each other?

A
  • metals lose electrons to form ions
  • metals do not react with each other (mix to form alloys)
    as they both would like to gain? electrons, so no reaction happens
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8
Q

what happens when a non metal forms an ion?

can non-metals react with each other?

A
  • non-metals gain electrons when forming ions

- yes, they form covalent bonds

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9
Q

what kind of solutions do metal oxides produce in water?

A

alkaline solutions

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10
Q

what kind of solutions do non metals form in water?

A

acidic solutions

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11
Q

what is a horizontal row in the periodic table called?

A

period

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12
Q

what is the column in the periodic table called?

A

group

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13
Q

what are ions?

A

an ion is an electrically charged particle formed when an atom or group of atoms lose or gain electrons

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14
Q

how do you represent an electron diagram?

A

draw a circle to represent each shell

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15
Q

how do ionic compounds form?

A
  • metal reacts with a non-metal
  • electrons are transferred from the metal atoms to the non-metal atoms
  • both achieve full outer shells (more stable)
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16
Q

what is the structure of an ionic compound?

A

giant ionic lattice (regular arrangement of positive and negative ions)

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17
Q

what are ionic bonds?

A

strong electrostatic forces between oppositely charged ions

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18
Q

what does the word ‘giant’ mean in ‘giant ionic lattices’?

A

the arrangement is repeated many times

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19
Q

what does the word ‘lattice’ mean in ‘giant ionic lattice’?

A

that the arrangement is regular and not random

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20
Q

what is a covalent bond?

A

a shared pair of electrons

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21
Q

how do covalent bonds form?

A

when two non-metal atoms share electrons in their outer shells

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22
Q

what does the intersection of a covalent bond diagram represent?

A

shared pair of electrons (bond itself)

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23
Q

When drawing a covalent bond diagram, how many shells are drawn?

A

Only the outer one

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24
Q

-

A

-

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25
Q

what is the bonding of simple molecules like?

A
  • electrostatic forces of attraction between nucleus and shared electron
  • covalent (electrostatic force) between atoms = strong
  • intermolecular forced between molecules = weak
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27
Q

how is the chemical formula of a giant ionic and covalent molecules shown?

A

using the empirical formula (simplest whole number ratio of atoms)

28
Q

what are giant covalent structures?

A
  • many repeating non-metal atoms joined by covalent bonds and arranged in a repeating regular pattern
  • called giant lattice
29
Q 
Order the following bonds depending on how high their melting/boiling points are :
Covalent Bond
Inter molecular forces 
Ionic 
Metallic
A

H Covalent
Ionic
Metallic
Inter Molecular Forces

30
Q

what do intermolecular forces do?

A

bonds molecules

31
Q

what is the strongest bond possible?

A

covalent bonds

32
Q

Do Giant ionic lattices have intermolecular forces, ionic bonds or covalent bonds?

A

ionic bonds

33
Q

Do Giant covalent lattices have intermolecular forces, ionic bonds or covalent bonds?

A
  • ONLY covalent bonds
34
Q

compare a giant ionic structure with a giant covalent structures

A
  • both are repeated in a regular pattern

- both are repeated many times

35
Q

State two limitations of ball and stick diagrams

A
  • size of atoms are exaggerated
  • length of bonds are exaggerated
  • suggests that electrons that make the bonds do not move
36
Q

Describe the structure in metals

A
  • forms giant metallic lattice

- regular pattern

37
Q

what is metallic bonding?

A
  • electrostatic forces of attraction between

delocalised electrons + positive metal ions

38
Q

Would it be easy to represent a giant covalent structure using a dot and cross diagram?

A

no because there are many atoms (almost too many to draw)

39
Q

What force acts between metal and non-metal ions?

A

electrostatic forces (ionic bonding)

40
Q

what is a delocalised electron?

A

an electron which is free to move about between different positive metal ions (within a giant metallic lattice)

41
Q

Why are metals good conductors of electricity and heat?

A

has delocalised electrons that can move around

42
Q

why are metal alloys stronger than pure metals?

A
  • the different sized atoms disrupt the regular arrangement of atoms (which stops the various layers from sliding over one another)
43
Q

how did Mendeleev arrange known elements in his periodic table?

A
  • in terms of their atomic mass

- in terms of similar chemical properties

44
Q

how did Mendeleev predict the properties of unknown elements?

A

by looking at the elements around it

45
Q

how was Mendeleev’s first periodic table arranged?

A

in rows and not columns

46
Q

why did Mendeleev arrange the periodic table in terms of atomic masses?

A

because protons had not been discovered yet

47
Q

who discovered that an element’s atomic number was actually the number of protons in its nucleus?

A

Henry Moseley

48
Q

Why had Mendeleev swapped tellurium and iodine around?

and why was he correct to do so?

A
  • he felt as if it ‘suited’ their chemical properties better
  • because tellurium had a higher number of protons to iodine (even though its mass was not)
49
Q

what was Mendeleev reluctant to believe?

A

that helium and argon were elements (because he thought that elements should be able to react with other elements - but they are inert)

50
Q

what do group 0 elements all have in common?

A

they are inert (do not react to other elements)

51
Q

do elements become more or less reactive as you go down in group 1 and 2?

A

more reactive

52
Q

do elements become more or less reactive as you go down in group 7?

A

less reactive

53
Q

is group 1 reactive?

A

VERY reactive

54
Q

is group 2 reactive?

A

yes, reactive

55
Q

is group 7 reactive?

A

VERY reactive

56
Q

is group 0 reactive?

A

no, not at all (inert)

57
Q

why are group 0 elements unreactive?

A

have complete outer shells, so they have no tendency to lose, gain, or share electrons.

58
Q

why are metals found in the left of the periodic table?

A

as they have fewer electrons in their outer shells

59
Q

Why do giant ionic lattices only have such a high boiling point?

A

as ionic bonds are very strong so a high amount of energy is needed to break them

60
Q

what are ionic bonds?

A

electrostatic forces of attraction between a non-metal and metal ion

61
Q

what bond joins monomers together to make polymers?

A

covalent bonds

62
Q

-

A

-

63
Q

what are polymers made of?

A

repeating monomers

64
Q

What evidence did Mendeleev have?

A
  • the atomic weights of the known elements, similar to our modern relative atomic masses
  • knowledge of the chemical reactions of different elements
  • knowledge of physical properties, such as melting points and boiling points

Chem C1-C3 (14 decks)

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