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chemistry > bonding and trends > Flashcards

bonding and trends Flashcards

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1
Q

types of elements in metallic bonds

A

between metal ions

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2
Q

type of elements in ionic bonds

A

between a metal and a non-metal

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3
Q

types of elements in covalent molecular bonds

A

non-metals

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4
Q

types of elements in covalent network bonds

A

non-metals

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5
Q

how are metallic bonds held together

A

an electrostatic attraction between the delocalised electrons and the positive ions

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6
Q

how are ionic bonds held together

A

an electrostatic attraction between the positive cations and the negative anions

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7
Q

how are covalent molecular bonds held together

A

an electrostatic attraction between the positive nuclei and the share pair of electrons

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8
Q

how are covalent network bonds held together

A

an electrostatic attraction between the positive nuclei and the share pair of electrons

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9
Q

what is the melting point of metallic bonding

A

high melting point due to the strong electrostatic attraction between the positive metal ions and the negative electrons

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10
Q

what is the melting point of ionic bonding

A

high melting point due to it having a strong electrostatic between the ions that a large amount of energy is required to remove it

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11
Q

what is the melting point of covalent molecular bonding

A

low melting point due to the electrostatic attraction in between the molecules being weak

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12
Q

what is the melting point of covalent network bonding

A

high melting point due to the intramolecular forces being strong so

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13
Q

how are metallic bonds formed

A

the valence electrons are removed from the cation’s and move freely with a 3D arrangement of the cations

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14
Q

how are ionic bonds formed

A

the electrons are transferred from the metals to the non-metals

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15
Q

how are covalent molecular bonds formed

A

two or more atoms will share their valence electrons to gain a full outer shell

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16
Q

how are covalent network bonds formed

A

two or more atoms will share their valence electrons to gain a full outer shell

17
Q

can metallic bonds conduct

A

it is conductivity due to the mobility of the delocalised electrons allowing the heat and electricity to move along the piece of metal

18
Q

can ionic bonds conduct

A

won’t conduct electricity if it is a solid since the electrons are in fixed positions but it can conduct if it is in a liquid or aqueous solution state since the electrons are free to move

19
Q

can covalent molecular bonds conduct

A

no, since conductivity requires a mobile charged particle to carry the charge. but there isn’t any charged particles in covalent molecular bonds since they are all neutral

20
Q

can covalent network bonds conduct

A

non-conductive except graphite, this is since all the electrons are used during intermolecular bonding. so there are no mobile electrons which mean it has a neutral charge

21
Q

why is metallic bonding malleable

A

the layers of positive ions can slip and slide past each other while keeping the metallic bond intact

22
Q

why are metallic bonding ductile

A

the layers of positive ions can slip and slide past each other while keeping the metallic bond intact

23
Q

why do metallic bonds have a hard property

A

the strong electrostatic attraction between the cations and the electrons. this makes it hard to separate the particles from one another

24
Q

what are some examples of metallic bonding

A

magnesium, sodium, potassium, lithium

25
Q

why are ionic bonding hard

A

hard due to the strong electrostatic between ion

26
Q

why are ionic bonds brittle

A

due to the orderly arrangement of the ions. this means that if the layers are forced to slide past each other, the like ions are pushed together, increasing repulsive forces and therefore shattering

27
Q

which state would you find covalent molecular bonds

A

most likely to be a liquid or gas at room temperature due to their low melting points.

28
Q

why are covalent molecular bonds soft

A

little force is required to push the molecules past each other

29
Q

why are covalent molecular bonds malleable

A

mainly in large molecules. they can be pushed past each other due to the weak forces between them

30
Q

why are covalent network bonds hard and brittle

A

the strongly bonded atoms are hard to disrupt so they are hard and brittle

31
Q

why are covalent molecules inert

A

due to the molecules all being neutral, there aren’t any particles that have a charge

32
Q

what are the five covalent network bonds

A

diamond, graphite, silcion carbide, silcion dioxide, boron nitride.

33
Q

what are some examples of ionic bonding

A

sodium oxide, potassium chloride, alumium hydroxide

34
Q

what are some examples of covalent molecular bonding

A

water, nitrogen oxide, carbon dioxide

35
Q

what types of substances dissolve in ethanol

A

types of substances that dissolve in ethanol are organic substances. due to ethanol being an organic substance, only organic substances can dissolve in ethanol. ethanol is organic since it contains carbon molecules. ethanol consists of both polar and non-polar bonds which are why it is organic. ethanol attracts non-polar substances.

36
Q

what are inorganic substances

A

any substance that doesn’t contain carbon. for example water. these are inorganic since they only have polar covalent bonds.

37
Q

what is a polar substance

A

Polar covalent bonding is a type of chemical bond where a pair of electrons is unequally shared between two atoms. polar bonds have a slightly positve and negative charge which attracts the polar water

38
Q

what is a non-polar substance

A

two atoms share a pair of electrons with each other

chemistry (4 decks)

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