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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
inorganic compounds
do not contain carbon
26
molecular compounds
have atoms bonded together via covalent bonds
27
ionic compounds
consist of two or more electrically charged atoms (ions) in which the overall charge is zero - ionic bonding
28
how are ions formed
due to changes in the electrons of an atom
29
cations
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
transitions metals and cations
can have varied charge in different complexes ie can give varied amounts of electrons and combine with different elements as a result
31
complex ion
consists of 2 or more atoms combined by covalent bonds with a net overall charge
32
monoatomic ion
an ion consisting of one atom
33
polyatomic ion
an ion consisting of more than one atom
34
monoatomic cations (write)
keep the name of the element, if more than. one type of cation is possible include the charge
35
monoatomic anions
change their endings to 'ide' fluorine- fluoride
36
oxyanions
complex ions in which an element combines with multiple oxygen atoms
37
naming oxoanions
most no. of oxygens - ate | one with fewer oxygens - 'ite'
38
hydrogen anions
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
perchlorate
CLO-4
40
hydrates
compounds containing a fixed number of water molecules
41
naming hydrates
add the polygonal prefix , then add 'hydrate'
42
binary molecules
compounds that consist of exactly two nonmetal elements
43
binary molecules naming
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
binary acids
usually 'h' and something else hydro_____ic acid
45
what must a substance contain in order to be considered an acid
hydrogen
46
oxoacid
when an oxyanion is protonated
47
oxyacid naming
ate - ic | ite - ous
48
trends in atomic radii
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
trends in ionic radius
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
electronegativity
the ability of an atom to attract electrons
51
trends in electronegativity
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
electron affinity
the energy change that occurs when an electron is added to an atom

TCD Chemistry (1 decks)

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