Bonding Flashcards

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

name, drawing and bond angle with 2bp 0lp

A
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11
Q

name, drawing and bond angle with3bp 0lp

A
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12
Q

name, drawing and bond angle with4bp 0lp

A
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13
Q

name, drawing and bond angle with3bp 1lp

A
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14
Q

name, drawing and bond angle with2bp 2lp

A
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15
Q

name, drawing and bond angle with5bp 0lp

A
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16
Q

name, drawing and bond angle with6bp 0lp

17
Q

name, drawing and bond angle with4bp 2lp

18
Q

name, drawing and bond angle with 4bp 0lp (nickel, platinum and pallidium)

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

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

positive charge
less electron density
less electronegative

25
what is hydrogen bonding
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
what causes permanent dipole-dipole forces
large differnce in electronegativity between two elements in a covalent bond * second strongest intermolecular force
27
what bond does permanent dipole-dipole forces create
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
what are van der waal forces and how are the caused
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
properties of vdw forces
weakest intermolecular forces larger the surface area the stronger the intermolecular force large molecules vdw's forces are stronger between molecules
30
order melting point from highest to lowest
- 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
31
what does d- mean
negative charge more electron density more electronegative