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elements of life > chemical bonding > Flashcards

chemical bonding Flashcards

1
Q

what are gas clouds made up of

A

a mixture of atoms and molecules together with the dust of solid material from old stars

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2
Q

how are gas clouds detected

A

by radio and infrared telescopes on Earth and by spectroscopic instruments carried by rockets

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3
Q

what do all noble gases have

A

a full outermost shell of electrons

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4
Q

how do other elements try achieving a full stable shell of electrons

A

by losing or gaining electrons

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5
Q

what does ionic bonding involve

A

metals reacting with non metals

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6
Q

when are ions formed

A

if the overall energy change when metals react with non metals is favourable

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7
Q

what happens in ionic bonding

A

electrons are transferred from the metal atoms to the non metal atoms giving the metal and non metal a stable electronic configuration of a noble gas

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8
Q

how are the ions held

A

by electrostatic attraction between oppositely charged ions

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9
Q

what do sodium and chlorine form

A

sodium chloride

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10
Q

what is an ionic bond

A

the bond between oppositely charged ions that attract each other strongly

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11
Q

how does a giant lattice form

A

in the solid compound each ion attracts many others of opposite charges to build up a lattice

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12
Q

what ions do group 1 elements form

A

+1 ions

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13
Q

what ions do group 2 elements form

A

+2 ions

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14
Q

what ions do group 3 elements form

A

+3 ions

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15
Q

what ions do group 6 elements form

A

-2 ions

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16
Q

what ions do group 7 elements form

A

-1 ions

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17
Q

write the formula for chromium (III) hydroxide

A
  • identify the atoms and charges a compound is made of - chromium (III) hydroxide is made of chromium (III) ions (Cr3+) and hydroxide ions (OH-)
  • work out the formulas so the charges balance - to balance the +3 charge you need 3 -1 charges
  • Cr(OH)3
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18
Q

why don’t non metallic elements form ions when they react

A

it isn’t energetically favourable to form ions

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19
Q

what happens when non metals react

A

electrons are shared between atoms of the element

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20
Q

what is covalent bonding

A

sharing of electrons

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21
Q

what is the result of covalent bonding

A

the resulting compound is mroe stable than the individual elements. shared electrons count as part of the outer shell of both atoms in the bond

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22
Q

what are covalent bonds

A

bonds formed by sharing electrons

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23
Q

how are the two atoms held together in covalent bonding

A

the positively charged nuclei are simultaneously attracted to the negatively charged shared electrons

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24
Q

what happens when electrons are shared

A

the atoms acheive more stable electrons

25
Q

what are bonding pairs

A

electron pairs which form bonds

26
Q

what are lone pairs

A

pairs of electrons not involved in bonding

27
Q

whats a double bond

A

when two pairs of electrons form a covalent bond e.g. oxygen and carbon dioxide

28
Q

whats a triple bond

A

when three pairs of electrons form a covalent bond e.g. nitrogen and hydrogen cyanide

29
Q

what are the three types of covalently bonded structures

A
  • polymers
  • simple molecular structures
  • covalent network structures
30
Q

describe the bonding in carbon monoxide

A

involves a triple bond. two of the pair of electrons are formed by the carbon and oxygen atoms each contributing one electron to the pair (ordinary covalent bonds)
however both electrons in the 3rd pair come from the oxygen atom (dative covalent bond)

31
Q

what is a dative covalent bond

A

both bonding electrons come from the same atom.

32
Q

how is a dative bond shown

A

by an arrow, it points away from the atom that is donating the pair of electrons

33
Q

how are the hydrogen atoms in a hydrogen molecule held together

A

their nuclei are both attracted to the shared electrons. both atoms are identical so the electrons are all shared equally

34
Q

what is the atomic core made up of

A

everything except the outer electrons

35
Q

what are the atomic cores attracted to in all atoms

A

to the shared electron pairs

36
Q

what is the charge of the atomic core of fluorine

A

Fluorine (2,7)
nucleus has a charge of +9 (has 9 protons)
innermost shell has a charge of -2 (2 electrons in the 1st shell)
the core has a charge of 7+ (9-2=7)

37
Q

how is the F2 molecule held together

A

the 7+ core charges are attracted to the negative charges on the shared electrons.

38
Q

what is often the case with atoms bonded together

A

they’re often different sizes.

39
Q

which are more attracted to the shared electrons - the smaller or bigger atom

A

the core of the smaller atom will be closer to the shared electrons and will exert a stronger pull on them.

40
Q

which atoms are also strongly attracted to the shared electrons

A

atoms with a greater core charge

41
Q

how do atoms attract bonding electrons

A

unequally

42
Q

why do atoms get a slightly positive or negative charge

A

one atom gets a slightly negative charge because it has a greater share of the bonding electrons. the other atom becomes slightly positively charged because it has lost its share in the bonding electrons

43
Q

what are slightly positive and slightly negative bonds called

A

polar bonds

44
Q

why is the O-H covalent bond polar

A

the two electrons in the bond are drawn closer to the oxygen atom athan the hydrogen atom

45
Q

what do metals and non metals form

A

ionic compounds

46
Q

what do non metals form

A

covalent compounds

47
Q

what do metals form

A

metallic compounds

48
Q

what is electronegativity

A

a measure of the ability of an atom in a molecule to attract electrons towards it. it measures an atoms attraction for bonding electrons

49
Q

an atom is highly electronegative if…

A

it has strong electron pulling powers in covalent bonds

50
Q

which atoms are more electronegative

A

if you exclude the noble gases the elements are more electronegative at the top of the group and at the RHS of the periodic table.

51
Q

what do highest electronegativities correspond with

A

reactive non metals with small atoms

52
Q

what do lowest electronegativites correspond with

A

reactive metals with large atoms

53
Q

describe polar bonds

A

they’re like covalent bonds with a bit of ionic character in them. ionic and covalent bonds are extreme forms of bonding - polar bonds are in between the two.

54
Q

the bigger the difference in electronegativity between the atoms ….

A

…. the more polar the bond and the greater the ionic character

55
Q

how do metal atoms acheive a full outer electron shell

A

metal atoms lose their outer electrons to form a lattice of regularly spaced positive ions. the outer electrons contribute to a sea of delocalised electrons which move freely through the lattice of cations

56
Q

what is each positively charged ion in the metal attracted to

A

the negatively charged delocalised electrons

57
Q

what is a metallic bond

A

the electrostatic attraction between the cations and the delocalised electrons

58
Q

what does the strength of the metallic bond depend on

A

the number of electrons per atom available for delocalisation

59
Q

more electrons lost =

A

= a more stronger bond

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