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Chemistry A-Level :p > Bonding > Flashcards

Bonding Flashcards

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1
Q

definition of ionic bonding

A

the strong electrostatic forces of attraction between oppositely charged ions to form the electron configuration of a noble gas

this occurs between metals and non metals

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2
Q

what do ions arrange themselves into

what is each ion in it attracted to

A

a giant ionic lattice

attracted to the oppositely charged electrons

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3
Q

what is one property of ionic compounds regarding mp/bp

A

they are solids at room temperature as they have very high melting and boiling points due to strong electrostatic forces of attraction within each oppositely charged ions in the giant ionic lattice. it takes a lot of energy to overcome the strong electrostatic forces of attraction

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4
Q

can ionic compounds conduct electricity?

A

they will not conduct electricity in a solid state as the ions are not free to move. they will conduct electricity when molten / aqueous

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5
Q

what are ionic compounds like density wise and why?

A

they are brittle

because they can easily shift layers, then the like ions (charges) will line up and repel

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6
Q

what 2 things increases the strength of ionic bonds ?

A

1) the greater ionic charge of the ions

2) the smaller the ionic radius

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7
Q

what is a covalent bond

A

a covalent bond is a shared pair of electrons between two non-metal atoms

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8
Q

how can a shared pair of electrons form a bond

A

the shared pair of electrons are attracted to the protons in the 2 nuclei , forming a covalent bond

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9
Q

what are atoms that are not part of covalent bonds called

A

lone pair of electrons

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10
Q

what is dative/coordinate bonding?

A

when an atom uses a lone pair of electron’s to form a covalent bond with an atom which has a vacant orbital

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11
Q

how do we represent a dative bond

A

an arrow

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12
Q

what must the atom donating the electrons have?

A

a lone pair of electrons (2 electrons not used in bonding)

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13
Q

what must the atom receiving the electrons in dative bonding must have ?

A

a vacant orbital

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14
Q

is a dative covalent bond the same as a normal covalent bond

they have the same…

A

yes

the same average bond enthalpy

(tells us the strength of the bond)

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15
Q

what is electronegativity

A

the ability/power of an atom to attract a pair of electrons in a covalent bond

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16
Q

what happens when the covalent bond consists of 2 atoms of the same element?

A

the shared pair of electrons are attracted to the nuclei equally

17
Q

why are noble gases not included in the electronegativity scale?

A

because they are unreactive

18
Q

what is electronegativity based on

what is the highest number for electronegativity

A

the pauling electronegativity scale

4

19
Q

what 3 factors does electronegativity depend on?

A

1) the size of the positive charge in the nucleus, moving left to right the number of protons increases which increases the attraction between nucleus and pair of electrons in the covalent bond

2) the atomic radius, from left to right the atomic radius decreases which means the closer the shared pair of electrons will be to the nucleus

3) shielding of nucleus by electrons in the inner shells, they screen the electrons in the outer shell from the positive charge in the nucleus

20
Q

what’s a dipole

A

a bond or molecule that has a difference in charge caused by a shift in electron density

21
Q

how to we show if a bond is polar

A

delta
+ -

22
Q

what is metallic bonding

A

strong electrostatic forces of attraction between positive metal ions and the sea of delocalised electrons

23
Q

what factors affect the strength of metallic bond

A

1) the ionic charge on the metal (higher =stronger metallic bonds)

2) number of delocalised electrons

3) the atomic radius (smaller = stronger )

24
Q

3 properties of metals

A

good conductors of electricity

high melting and boiling points

metals are malleable and ductile (layers of ions

25
Q

what does covalent bonding lead to the formation of

A

the formation of either simple or giant molecules

26
Q

name 3 types of intermolecular forces in order of strength

A

1) van der waals forces between molecules

2) permanent dipole-dipole forces between molecules

3) hydrogen bonding between molecules

27
Q

what’s van der waals forces

A

electrons are constantly moving from place to place so charge can change distributed at any time

this means one side of the
molecule can suddenly become more negative than the other side if the electrons have moved closer to that side

(this is called a temporary dipole )

28
Q

how will a temporary dipole affect the neighbouring atoms and charge spread

(van der walls forces)

A

a temporary dipole in one molecule induces a dipole in the neighbouring molecules as it repels the electrons to the other side (induced dipole)

now there is a force of attraction between the $+ $- called van der waal forced

29
Q

what intermolecular force do all molecules have

A

van der waal force

30
Q

what affects the size of van der waal forces? (2)

A
  • size/mr of the molecule (bigger molecule=more van der waals forces between molecules)
  • surface area contact
31
Q

what is permanent dipole-dipole forces between molecules

A

it only occurs between molecules which are polar

(a polar bond is a difference in electronegativity between atoms

there is a attraction between the oppositely charged deltas on the neighbouring molecules

32
Q

what is hydrogen bonding

A

this is very similar to permanent dipole-dipole bonding however this only occurs with polar molecules which have hydrogen directly bonded to nitrogen , oxygen and fluorine

this is because they are the most polar molecules

hydrogen and these elements have a huge difference in electronegativity and as a result pull the pair of electrons in the covalent bond very strongly towards themselves

this leaves hydrogen very delta positive

the lone pair of electrons in the neighbouring molecule containing nitrogen, oxygen and fluorine is then attracted to the hydrogen

Chemistry A-Level :p (14 decks)

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