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TCD Chemistry > Lecture 1 and 2 > Flashcards

Lecture 1 and 2 Flashcards

1
Q

Atom

A

The smallest unit of matter

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2
Q

Neutron

A

Have no charge
Have mass
reside in the nucleus

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3
Q

Protons

A

Have a positive charge
have equivalent mass to neutrons
reside in the nucleus

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4
Q

Electron

A

have a negative charge
have mass 1/1836 of protons
reside in the nucleus

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5
Q

In a neutral atom

A

the number of protons = no. of electrons

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6
Q

Atomic number

A

the number of protons in the nucleus

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7
Q

mass number

A

number of protons and neurtrons in the nucleus

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8
Q

Periodic table arrangement

A

vertical columns ; groups - arranged by trends in chemical reactivity

horizontal rows ; periods -

s,p,d,f blocks based on where the elements outer electrons lie

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9
Q

group 1

A

alkali metals
soft metals
react to release hydrogen when put in water

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10
Q

group 2

A

alkaline earth metals

also react with water and release hydrogen

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11
Q

group 17

A

halogens
very reactive gases
combine with alkali metals to form salt

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12
Q

group 18

A

noble gases
inert , unreactive gases
have a full outer shell of electrons

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13
Q

moles

A

the amount of substance that contains the same amount of atoms/particles/molecules as there are atoms in 12 grams of carbon 12

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14
Q

molar mass

A

the mass in grams of one mol of any substance

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15
Q

molar mass

A

mass in grams per mole

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16
Q

number of atoms/molecules/ions

A

no. of moles x avogadros number

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17
Q

octet rule

A

when atoms combine, their electrons arrange such that every atom has 8 electrons on their outer shell

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18
Q

valence electrons

A

the electrons on the outer shell of an atom that are involved in completing the octet rule

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19
Q

valence

A

the minimum number of electrons that an atom must lose or gain in order to get to the octet rule

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20
Q

group 1 reactivity

A

all have 1 electron on outer shell - hence reactivity is similar

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21
Q

covalent bond

A

two atoms share electrons

22
Q

reactivity

A

building atoms into matter

the atoms are arranged in space by reactions mediated by electrons
atoms react to obtain the most stable form - ie lowest energy configuration of electrons

23
Q

compounds

A

2 or more elements in specific combination

24
Q

organic compounds

A

contain carbon

25
Q

inorganic compounds

A

do not contain carbon

26
Q

molecular compounds

A

have atoms bonded together via covalent bonds

27
Q

ionic compounds

A

consist of two or more electrically charged atoms (ions) in which the overall charge is zero - ionic bonding

28
Q

how are ions formed

A

due to changes in the electrons of an atom

29
Q

cations

A

metals are generally cations
they tend to lose electrons

for groups one and two the charge of the cation Is the same as the group number

they have one/two electrons on outer shell - they want to lose these electrons when bonding

they lose the amount of electrons on their outer shell and as a result have an excess of protons - therefore they are positively charged

30
Q

transitions metals and cations

A

can have varied charge in different complexes

ie can give varied amounts of electrons and combine with different elements as a result

31
Q

complex ion

A

consists of 2 or more atoms combined by covalent bonds with a net overall charge

32
Q

monoatomic ion

A

an ion consisting of one atom

33
Q

polyatomic ion

A

an ion consisting of more than one atom

34
Q

monoatomic cations (write)

A

keep the name of the element, if more than. one type of cation is possible include the charge

35
Q

monoatomic anions

A

change their endings to ‘ide’

fluorine- fluoride

36
Q

oxyanions

A

complex ions in which an element combines with multiple oxygen atoms

37
Q

naming oxoanions

A

most no. of oxygens - ate

one with fewer oxygens - ‘ite’

38
Q

hydrogen anions

A

anions with h+ added are less negative by one because of the plus

add hydrogen to the beginning of the element eg

hydrogen sulphide

39
Q

perchlorate

A

CLO-4

40
Q

hydrates

A

compounds containing a fixed number of water molecules

41
Q

naming hydrates

A

add the polygonal prefix , then add ‘hydrate’

42
Q

binary molecules

A

compounds that consist of exactly two nonmetal elements

43
Q

binary molecules naming

A

use polygonal prefixes to denote the no. of atoms - then write the name of the first element followed by the second element ending in ‘ide’

44
Q

binary acids

A

usually ‘h’ and something else

hydro_____ic acid

45
Q

what must a substance contain in order to be considered an acid

A

hydrogen

46
Q

oxoacid

A

when an oxyanion is protonated

47
Q

oxyacid naming

A

ate - ic

ite - ous

48
Q

trends in atomic radii

A

increases as you move down the periodic table
extra electrons being added and more shells hence the radius increases

decreases as you move across the periodic table
because they all have a full outer shell of electrons - there is more columb force pulling the negative and positive charges together

49
Q

trends in ionic radius

A

aka the size of an ion of a given element

the trends are the same as atomic radius, for the same reasons however the metals (L) become smaller as they lose electrons and the none metals become bigger

50
Q

electronegativity

A

the ability of an atom to attract electrons

51
Q

trends in electronegativity

A

elements with an almost full outermost shell will want electrons the most - aka a high electronegativity

elements with lots of full inner shells (towards the bottom of the periodic table) will want electrons the least

low electronegativity

52
Q

electron affinity

A

the energy change that occurs when an electron is added to an atom

TCD Chemistry (1 decks)

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