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Applied science CHEM > unit 1 > Flashcards

unit 1 Flashcards

1
Q

relative mass of a proton

A

1

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2
Q

relative mass of a neutron

A

1

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3
Q

relative mass of an electron

A

1/2000

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4
Q

relative charge of a proton

A

+1

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5
Q

relative charge of a neutron

A

0

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6
Q

relative charge of an electron

A

-1

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7
Q

define mass number

A

number of protons + number of neutrons

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8
Q

define atomic number

A

number of protons

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9
Q

what is the principle quantum number

A

energy levels are identified by a number, the larger the number of n the further away from the nucleus and higher the energy level it is

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10
Q

what do each shell contain

A

atomic orbitals

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11
Q

define wave particle duality

A

electrons can behave like a wave or particle

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12
Q

4 types of orbitals

A

s p d f

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13
Q

features of s orbital

A

spherical. holds 2 electrons max

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14
Q

features of p orbital

A

3d dumbbell shape 6 electrons max

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15
Q

define subshells

A

a group of the same type of orbital with a shell
(Each new shell gains a new type of sub shell)

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16
Q

max electrons s subshell can hold

A

2

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17
Q

max electrons p subshell can hold

A

6

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18
Q

max electrons d subshell can hold

A

10

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19
Q

max electrons f subshell can hold

A

14

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20
Q

max electrons in main energy level 1

A

2

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21
Q

max electrons in main energy level 2

A

8

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22
Q

max electrons in main energy level 3

A

18

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23
Q

max electrons in main energy level 4

A

32

24
Q

what is Aufbau principle

A

Start at the lowest energy level (shell) and add electrons one at a time.

Fill each sub level before starting the next

25
Q

define isotope

A

atoms of the same element with the same number of protons but different numbers of neutrons

26
Q

Define ionic bonding

A

The electrostatic attraction between oppositely charged ions

27
Q

Define Hunds rule

A

Fill each orbital with one electron at a time before pairing electrons

28
Q

define groups

A

columns on a periodic table
elements in a group have similar properties

29
Q

define electron transfer

A

occurs between metals and non metals

30
Q

in ionic bonding metals electrons and become ions, non metals electrons and become ions

A

lose, positive
gain, negative

31
Q

3 properties of ionic bonding

A

strong electrostatic forces (in all directions between oppositely charged ions)

high melting + boiling points

when melted or dissolved in water ionic compounds can conduct electricity (ions are free to move + carry current)

32
Q

diamond features

A

all atoms in the structure are linked by strong covalent bonds

high melting points

each carbon forms 4 covalent bonds so very hard

Doesn’t conduct electricity

Tetrahedral shape

33
Q

graphite features

A

each carbon form to 3 others forming layers

layers slide over each other because there no covalent bonds between layers

soft and slippery

1 electron from 1 carbon is delocalised which allows conduction of heat + electricity

34
Q

define macromolecule

A

giant covalent bonds

35
Q

covalent bonding molecules properties

A

shared pair of electrons

low melting and boiling point (weak intermolecular forces easier to break)

doesn’t conduct electricity (molecules don’t have overall charge, no free electrons or ions)

36
Q

metallic bonding features

A

giant structures of atoms in a regular pattern

loose electrons in outer shell (free to move)

‘sea’ of delocalised electrons

Strong electrostatic attraction between negatively charged electrons that holds structure together

37
Q

how to work out Mr

A

add mass number of all elements present together

38
Q

%mass equation

A

mass of element/mass of compound x 100

39
Q

%yield equation

A

amount of product (actual)/max of potential (theoretical) x 100

40
Q

define empirical formula

A

simplest whole number ratio

41
Q

What is a Dative covalent bond

A

The atoms supplies both the shared pair of electrons to the covalent bond

42
Q

What is lone pair of electrons

A

Outer shell pair of electrons this is not involved in chemical bonding

43
Q

The Of a solution is a measure of how much Is dissolved of .

A

Concerntrate , solute, per unit, solvent

44
Q

Concerntration equation

A

Amount of solvent (moles)/ volume of solute (dm^3)

Mass of solid / volume of liquid

45
Q

What is solute measured in

A

Moles (amount)

46
Q

Volume of solvent is measured in

A

Dm^3

47
Q

conc measured in

A

moldm^3

48
Q

1 ml to cm

A

1cm

49
Q

1000ml to litre

A

1litre

50
Q

1000ml to dm^3

A

1dm^3

51
Q

What did dimitri Mendeleev do

A

Arranged elements by atomic weight

Left gaps for missing elements

Elements in the same group have similar properties

52
Q

What did Henry Moseley do

A

Arranged period group in order of increasing atomic number (related to atomic mass)

53
Q

Define periodicity

A

Variation of properties of elements with changing atomic number

54
Q

What is First ionisation energy

A

The energy required to remove one electron from each atom in one mole of atoms in the gaseous state ( from 1 mole of 1+ ions)

Na(g) -> Na(g) + e-

Nuclear charge increases (more attraction) harder to lose electron

55
Q

What is titration

A

Neutralisation coloured water to colourless to see conc of solution

Applied science CHEM (1 decks)

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