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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

what is ionic bonding

A

strong electrostatic forces of attraction between oppositely charged ions

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2
Q

what are the properties of ionic bonds

A

conduct electricity when melted or in solution
high melting points
second strongest structure and bond

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3
Q

what is a covalent bond

A

shared pair of electrons

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4
Q

what is a covalent lattice

A

many strong covalent bonds (shared pair of electrons)

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5
Q

what is a dative covalent bond

A

shared pair of electrons with both electrons supplied by one atom

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6
Q

properties of covalent bonds

A

strongest structure and bond
don’t conduct electricity apart from graphite (has delocalised electrons and van der waals forces)

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7
Q

what are metallic bonds

A

strong electrostatic forces of attraction between delocalised electrons and positively charged ions.

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8
Q

properties of metallic bonds

A

conduct electricity
have high melting points
ductile and malleable
third strongest structure and bond

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9
Q

what do lone and bonding pairs do to each other

A

repel each other
lone pairs repel 2-2.5 degrees more than bp

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10
Q

2bp 0lp

A

name : linear
bond angle : 180
diagram : x—-y—-x

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11
Q

3bp 0lp

A

name : trigonal planar
bond angle : 120
diagram :

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12
Q

4bp 0lp

A

name : tetrahedral
bond angle : 109.5
diagram :

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13
Q

3bp 1lp

A

name : trigonal pyramidal
bond angle : 107
diagram :

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14
Q

2bp 2lp

A

name : bent
bond angle : 104.5
diagram :

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15
Q

5bp 0lp

A

name : trigonal bypyramidal
bond angle : 120 and 90
diagram :

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16
Q

6bp 0lp

A

name : octahedral
bond angle : 90
diagram :

17
Q

4bp 2lp

A

name : square planar
bond angle : 90
diagram :

18
Q

4bp 0lp (nickel, platinum and pallidium)

A

name : square planar
bond angle : 90
diagram :

19
Q

what is electronegativity

A

ability of an atom to attract a bonding pair of electrons in a covalent bond

20
Q

what affects electronegativity

A

atomic radius and number of protons

21
Q

what element is most electronegative

A

fluorine

22
Q

what are polar bonds

A

bonds that have a permanent uneven distribution of electron density caused by a large difference in electronegativity

23
Q

what causes symmetrical molecules

A

the electronegative elements pull in equal and opposite directions so cancel out

24
Q

what does d- mean

A

negative charge
more electron density
more electronegative

24
Q

what does d+ mean

A

positive charge
less electron density
less electronegative

25
Q

what is hydrogen bonding

A

the electrostatic attraction in a hydrogen bond is between the lone pair on the N/O/F and the d+ hydrogen
is between molecules
* strongest intermolecular foce

26
Q

what causes permanent dipole-dipole forces

A

large differnce in electronegativity between two elements in a covalent bond
* second strongest intermolecular force

27
Q

what bond does permanent dipole-dipole forces create

A

polar bonds where one of the elements usually N/O/F/Cl id d- as they are more electronegative and the less electronegative element is d+

28
Q

what are van der waal forces and how are the caused

A

caused by a random movement of electrons causing a temporary dipole in that molecule (with a d- and d+)
the partial charge causes electron density to be attracted/repelled in other nearby molecules which induces a dipole

29
Q

properties of vdw forces

A

weakest intermolecular forces
larger the surface area the stronger the intermolecular force
large molecules vdw’s forces are stronger between molecules

30
Q

order melting point from highest to lowest

A
  • diamond graphite as they are giant covalent lattices bonds to break
  • metal and non metal is a giant ionic lattice forces of attraction to overcome
  • metals are giant metallic lattices forces of attraction to overcome
    *2 or more non metals bonded together are simple molecular forces of attraction between molecules to overcome
  • hydrogen bonding
  • permanent dipole dipole
  • van der waals

Chemistry (24 decks)

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