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chemistry: physical chemistry 1 > bonding > Flashcards

bonding Flashcards

1
Q

what is metallic bonding?

A

strong attraction between positive ions and negative sea of electrons

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2
Q

what are the properties of metals?

A

● good conductors of electricity

● good conductors of heat

● malleable

● ductile

● strong

● high melting point

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3
Q

why are metals a good conductor of electricity?

A

delocalised elections can move through structure to carry the charge

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4
Q

what does malleable mean?

A

can be beaten into shape

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5
Q

what does ductile mean?

A

can be pulled into thin wires

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6
Q

what does the strength of a metallic bond depend on?

A

● charge of ion ↑

● size of ion ↓

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7
Q

why do metals have high melting points?

A

lots of energy required to overcome strong metallic bonds

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8
Q

smaller ions will attract electrons…

A

more strongly as they are closer to nucleus

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9
Q

if nuclear charge is bigger…

A

stronger attraction

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10
Q

if there are more delocalised electrons…

A

more forces of attraction

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11
Q

what is ionic bonding?

A

● electrons are transferred

● metal and non metal

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12
Q

what is the ionic bonding structure?

A

● giant ionic lattice

● held together by strong electrostatic forces of attraction between oppositely charged ions

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13
Q

what are the properties of giant ionic lattices?

A

● electrical conductivity

● shatters easily / brittle

● high melting point

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14
Q

when are ions free to move in giant ionic lattices?

A

● when molten or aqueous ions are free to move and can conduct electricity

● when solid ions are not free to move and cannot conduct electricity

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15
Q

explain strength in giant ionic lattices

A

● shatters easily / brittle

● any disruption to structure that makes positive ions or negative ions align will cause them to repel and shatter

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16
Q

explain melting point in giant ionic lattices

A

● high

● strong electrostatic forces of attraction between oppositely charged ions

● force acts in all directions

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17
Q

what does the strength of an ionic bond depend on?

A

● the larger the charge of ion, the stronger the attraction

● the smaller the ion, the stronger the attraction

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18
Q

what is covalent bonding?

A

● shared pair of electrons

● strong

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19
Q

what are properties of simple covalent molecules?

A

● melting point and boiling points are low

20
Q

what is the orbital theory?

A

covalent bonds are formed when orbitals, each containing 1 electron, overlap

21
Q

what is the octet rule?

A

● tendency to prefer 8 electrons in outer shell

● we do not consider p and f electrons

● only s and d are involved

22
Q

what is coordinate bonding?

A

● in most covalent bonds, each atom provides 1 electron

● but in some bonds, one atom provides both electrons

● shared pair of electrons but both electrons come from same atom

● have exactly same strength and length as ordinary covalent bonds once they are formed

23
Q

what are coordinate bonds represented by?

A

● →

● points towards atom accepting bond

24
Q

what is electronegativity?

A

the power of an atom to attract the electron density in a covalent bond towards itself it

25
Q

what are the factors affecting electronegativity?

A

● nuclear charge - more protons, stronger attraction between nucleus and bonding pair of electrons

● atomic radius - closer to the nucleus, stronger attraction between nucleus and bonding pairs of electrons

● shielding - less shells of electrons between the nucleus and the electrons less shielding (less repulsion), stronger attraction between nucleus and bonding pair of electrons

26
Q

what is the trend of electronegativity down a group?

A

● decreases

● nuclear charge increases, but atomic radius increases and more shielding

● therefore, less attraction between nucleus and bonding pair of electrons

27
Q

what is the trend of electronegativity across a period?

A

● increases

● nuclear charge increases, but atomic radius decreases and shielding stays the same

● therefore, stronger attraction between nucleus and bonding pair of electrons

28
Q

explain electronegativity in bonds between identical atoms

A

● electrons are shared equally

● no difference in electronegativity

● non polar

29
Q

explain electronegativity in bonds between different atoms

A

● different electronegativity

● one will pull the electrons closer to its end

● it will have a slight negative charge (δ⁻)

● other will have slight positive charge (δ⁺)

● leads to a charge difference called a dipole

● dipoles can be permanent

● greater the difference in electronegativity, the greater the polarity of the bond

30
Q

what are some elements with high electronegativity?

A

● O

● F

● N

● Cl

31
Q

what is polarity?

A

about unequal sharing of electrons between atoms that are bonded covalently

32
Q

how is bond polarity represented?

A

an arrow with a line at the end pointing to more electronegative atom

33
Q

explain non polar molecules

A

● they take into account all of the dipoles across the bonds of molecule

● for molecules that are symmetrical, dipoles of any bond within the molecule can cancel out

34
Q

explain polar molecules

A

● not all molecules containing polar bonds are polar overall

● if bond dipoles cancel each other the molecule isn’t polar

● if there is a ‘net dipole’ the molecule will be polar

35
Q

is the molecule NH3 polar?

A

yes, shape of molecules means the dipoles do not cancel each other out

36
Q

is the molecule CCl4 polar?

A

no, although it contains polar bonds the molecules is symmetrical so the dipoles cancel out

37
Q

what do intramolecular bonds affect?

A

chemical bonds

38
Q

what do intermolecular forces affect?

A

physical properties

39
Q

what are the 3 types of forces between molecules?

A

● van der waals forces: act between all atoms and molecules

● dipole-dipole forces: act only between certain types of molecules

● hydrogen bonding: acts only between certain types of molecules

40
Q

explain van der waal forces

A

● as electrons are constantly moving an instantaneous dipole can occur in an atom or molecule that isn’t polar

● this is where electron density shifts to one end of the molecule

● when instantaneous dipole comes close enough to another molecule it induces a new dipole in neighbouring molecule

● now also polar, the 2 are attracted to each other

41
Q

what affects strength of van der waal forces?

A

● number of electrons

● more electrons means the stronger the instantaneous dipole will be

42
Q

explain boiling point and van der waal forces

A

● electrons increase

● van der waal forces increase

● boiling point increases

43
Q

explain dipole-dipole forces

A

● polar molecules have permanent dipoles

● molecule will always have a negatively and positively charged end

● forces between two molecules that have permanent dipoles are called permanent dipole - dipole forces

● δ+ end of the dipole in one molecule and the δ- end of the dipole in a neighbouring molecule are attracted towards each other

44
Q

explain boiling point and dipole-dipole forces

A

extra attraction between dipoles means more energy must be put in to separate molecules so you get a higher boiling point than expected for a given mass

45
Q

explain hydrogen bonding

A

● force not bond

● same characteristics as covalent bond and dipole-dipole forces

● 1/10 strength of regular covalent bond

● only occurs when hydrogen is bonded covalently to fluorine, nitrogen or oxygen

● hydrogen has large charge density (small) and F, N and O are highly electronegative

● bond is polarised so that H of one molecule forms a weak bond with F, N or O of another molecule

● often attracted to lone pairs on O and N

chemistry: physical chemistry 1 (5 decks)

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