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chemistry > Foundations in chemistry > Flashcards

Foundations in chemistry Flashcards

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1
Q

What is the real active mass of an electron proton and neutron

A

Proton is 1
Neutron is 1
Electron is 1/1836

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2
Q

What is an isotope

A

Atoms of the same element with the same number of protons but a different number of neutrons

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3
Q

What is relative isotopic mass

A

Mass of an atom of an isotope compared with 1/12th mass of carbon 12

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4
Q

What is relative atomic mass

A

Weighted mean mass of an atom of an element compared with 1/12th mass of carbon 12

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5
Q

How many electrons are on each shell

A

1 has 2 electrons
2 has 8 electrons
3 has 18 electrons
4 has 32 electrons

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6
Q

What is a orbital

A

A region of space around the
Nucleus that can hold two electrons with paired spins

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7
Q

What orbitals do each energy levels have

A

1st has only s
2nd has s and p
3rd has s , p and d
4th has s , p , d and f

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8
Q

How many orbitals do each sub shell have

A

S has 1
P has 3
D has 5
F has 7

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9
Q

Why do electrons in the same orbital get drawn as oppositely facing arrows

A

The negative electrons repel each other and it also indicated the electrons spin

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10
Q

What is the electron configuration of carbon

A

1s2 2s2 2p2

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11
Q

how to write short hand electron configuration

A

replacing orbitals with the most recent preceding noble gas’s known electron configuration

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12
Q

what is the shorthand configuration of chlorine

A

[Ne]3s²3p5

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13
Q

what are the noble gas facts

A

full valence electron shells
monoatomic non metal gases at room temp
very stable
high ionising energies
do not combust
low bp

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14
Q

what is ionic bonding

A

electrostatic attraction between oppositely charged ions

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15
Q

what happens to electrons in ionic bonding

A

they are transferred

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16
Q

what is a covalent bond

A

shared pair of electrons

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17
Q

What is a dative covalent bond

A

when a shared pair of electrons that have been donated by only of the bonded atoms for example NH4

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18
Q

What groups can break the octet rule

A

5-7

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19
Q

In double and triple covalent bonds all atoms have the structure of the…

A

Nearest noble gas

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19
Q

How is expanding the octet possible

A

In the. 3rd shell when a d sub shell becomes available

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20
Q

How do dative covalent bonds usually occur

A

When a compound reacts with a H+ ion

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21
Q

What is the name and bond angle of a covalent molecule with 2 electron pairs

A

Linear
180

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22
Q

What is electron repulsion theory

A

The shape of a molecule is determined by the number of electron pairs as electrons repel each other

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23
Q

What is the name and bond angle of a molecule with 3 electron pairs

A

Triagonal planar
120

24
Q

What is the name and bond angle of a molecule with 4 electron pairs

A

Tetrahedral
109.5

25
Q

What is the name and bond angle of a molecule with 5 electron pairs

A

Trigonal bipyramidal
120/90

26
Q

What is the name and bond angle of a molecule with 6 electron pairs

A

Octaheadral
90

27
Q

What is the name and bond angle of a molecule with 1 lone pair

A

Pyramidal
107

28
Q

What is the name and bond angle of of a molecule with 2 lone pairsb

A

Non linear
104.5

29
Q

what is electronegativity

A

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

30
Q

What are examples of very electronegative elements

A

oxygen, florine, chlorine, nitrogen etc

31
Q

what are factors affecting electronegativity

A

atomic charge
distance from the nucleus
electron shielding

32
Q

what is a HCl bond known as

A

polar covalent bond

33
Q

what must a molecule be for it to be polar

A

asymmetrical

34
Q

what does a polar molecule form

A

a dipole

35
Q

why are symmetrical molecules non polar

A

the dipoles cancel each other

36
Q

do lone pairs cause symmetrical or asymmetrical molecules

A

asymmetrical

37
Q

what is an intermolecular force

A

an attractive force between neighbouring molecules

38
Q

what are the 3 types of intermolecular forces

A

-permanent dipole-dipole interactions
-london forces
-hydrogen bonds

39
Q

what is the strongest and weakest intermolecular force

A

hydrogen is strongest
london in weakest

40
Q

explain a permanent dipole force

A

-Its a weak attractive force between permanent dipoles in neighbouring polar molecules
-The permanent dipole of one molecule attracts the permanent dipole of another

41
Q

explain london forces

A

-They act between all molecules, whether they are polar or non polar
-Electrons might find themselves towards one side of the molecule because they are mobile, forming a temporary dipole
-This creates induced dipoles which are attracted to the temporary dipoles

42
Q

explain hydrogen bonding

A

-Electrostatic forces of attraction between a proton deduced of electrons attached to an electronegative atom and the lone pair of another electronegative atom

43
Q

why is ice less dense as a solid

A

the hydrogen bonds hold the H2O molecules in an open lattice shape as a solid, bit as they melt the molecules move closer together

44
Q

what elements does hydrogen bonding happen to with hydrogen

A

Nitrogen, Oxygen and Florine

45
Q

What is metallic bonding

A

The electrostatic attraction between positive metal ions and delocalised electrons

46
Q

What are the properties of giant metallic lattices

A

High mp and bp
Good electrical conductors
Malleable and ductile

47
Q

What do giant metallic lattices have high melting points and boiling points

A

Strong electrostatic attraction between positive metal ion and delocalised electrons which require a lot of energy to overcome

48
Q

Why are giant metallic lattices good electrical conductors

A

Delocalised electrons are free to move and carry a charge

49
Q

Why are giant metallic lattices malleable and ductile

A

The ions are able to move past each other into new positions whiteout breaking metallic bonds

50
Q

What is an alloy

A

A mixture of metals

51
Q

what is an ionic lattice

A

regular repeating pattern of oppositely charged ions

52
Q

what are the properties of ionic compounds

A

-Conductors when molten
-High mp and bp
-Soluble in polar solvents

53
Q

explain why ionic lattices are conductors when molten

A

ions are free to move through the structure

54
Q

explain why ionic lattices have high melting and boiling points

A

electrostatic attraction between oppositely charged ions is so strong large amounts of energy are needed to overcome

55
Q

what can increase electrostatic attraction in ionic compounds/lattices

A

higher ion charge

56
Q

explain why ionic lattices are soluble in polar solvents

A

polar molecules break down the lattice by surrounding each ion to form a lattice; positive ion in solvent to negative ion in lattice, and negative ion in solvent to positive ion in lattice

57
Q

What are properties of simple molecular substances

A

-weak and soft when solid due to intermolecular forces
-don’t conduct electricity as not charged
-soluble in non polar solvents because London forces form between the solvent and molecule

58
Q

what are the differences between graphite and diamond

A

graphite can conduct electricity but diamond cannot

chemistry (4 decks)

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