Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Elements of life > Flashcards

Elements of life Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

what is the bonding and structure of each group in the periodic table

A

1-3=metallic
4-7=covalent

1-4=giant
5-7=molecular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

how have shells of electrons of electrons been proven to exist

A

atoms produce emission spectra

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what does an atomic emission spectrum look like

A

coloured lines on a black background

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what does an atomic absorption spectrum look like

A

black lines on a coloured background

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what does the atomic number of an element tell you about it

A

number of protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what is special about P orbitals

A
  • P subshells always contain 3 P orbitals
  • shells 2 upward contain P orbitals
  • P orbitals are shaped like a figure of 8
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

NO3-

A

Nitrate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

SO4 2-

A

sulfate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

CO3

A

carbonate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

OH-

A

hydroxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

NH4

A

ammonium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

HCO3

A

hydrogen carbonate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

how many sets do double bonds count for

A

one

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

how does an emission spectrum occur

A
  • electrons excited to a higher energy level by heating

- when they fall back down, they emit light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

why is the bond angle of water 104.5degrees

A

4 sets of electrons with two lone pairs

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

how many electrons can a D subshell hold

A

10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what bond is between 2 non-metals

A

covalent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what is the equation that links moles, mass and relative atomic mass

A

mass=molesXrelative atomicmass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what is special about the S orbitals

A
  • spherical

- found in every shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

which two elements have the same atomic emission spectra

A

none. all elements have unique energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

on an a-level periodic table what shows you the mass of one mole

A

relative atomic mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

what is a dative covalent bond

A
  • shared pair electrons

- both electrons come from the same atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

what is the bond angle and shape of an atom with 4 sets of electrons

A

109.5

tetrahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

how do you predict the amount of a product in a reaction

A

1-work out moles of known substance 2-work out mole of unknown substance using mole ratio 3.work out mass of unknown substance, m=nXAr

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

what bond is between a metal and non metal

A

ionic

26
Q

Cu2+

A

copper

27
Q

Zn2+

A

zinc

28
Q

Pb2+

A

lead

29
Q

Fe2+

A

iron(II)

30
Q

Fe3+

A

iron(III)

31
Q

how do you calculate the % yield

A

%yield=(actual amount of product-divide- expected amount of product)X100

32
Q

what is the bond angle and shape of an atom with 3 sets of electrons

A

120degrees

planar

33
Q

how much does each lone pair reduce the angle by

A

2.5 degrees

34
Q

in what order do the subshells fill up in

A

s, p, d, f

35
Q

why does nuclear fusion require a high temperature

A

to overcome the repulsion of the nuclei

36
Q

what is the empirical formula

A

simplist ratio of atoms in the compound

37
Q

what is the equation that links: speed of light, wavelength, frequency

A

speed of light= wavelength x frequency

38
Q

what is the bond angle and shape of an atom with 2 sets of electrons

A

180

linear

39
Q

why does 4s fill up before the 3d subshell

A

because it has a lower energy level

40
Q

what is an orbital

A
  • a 95% probability surface of finding an electron

- 95% of the time an electron will be found in a particular region of the orbital

41
Q

what is bonding between: calcium oxide, magnesium, carbon dioxide, silicon

A

ionic
metallic
covalent
covalent

42
Q

what is the equation that links: planks constant, frequency, energy gap

A

Energy gap= frequency X planks constant

43
Q

what is a precipitation reaction

A

happens when two solutions react together and form an insoluble solid, which is called a precipitate

44
Q

give 3 key points of ionic bonding

A
  • ionic bonds are strong so have a high melting points

- they do not not conduct electricity as solids

45
Q

HCO3-
NO3-
CO3 2-
SO4 2-

A

hydrogen carbonate
nitrate
carbonate
sulfate

46
Q

hydrogen carbonate
nitrate
carbonate
sulfate

A

HCO3-
NO3-
CO3 2-
SO4 2-

47
Q

what is the melting point of ionic bonding

A

ionic bonds are strong. so ionic bonds have high melting point

48
Q

what is the melting point of metallic bonding

A

strong attractions between metal ions and delocalised electrons therefore melting point is high

49
Q

what is the melting point of giant covalent networks

A

lots of strong covalent bonds therefore high melting points

50
Q

what is the conductivity of ionic bonding

A
  • do not conduct as solids because ions cannot move

- conduct as solutions and liquids because ions can move

51
Q

what is the conductivity of metallic bonding

A

delocalised electrons are free to move, so metals conduct electricity

52
Q

what is the conductivity of giant covalent networks

A

only conducts if it contains delocalised electrons

53
Q

what is the trend in first ionisation energy down group 1

A

decreases

54
Q

what is the trend in first ionisation energy across period 3

A

increases

55
Q

what is ionisation energy

A

energy required to remove one electron from each atom in a mole of gaseos atoms

56
Q

what are some notes on ionisation energy

A
  • looses one electron at a time
  • electrons need energy to be excited to a very high energy level and leave
  • removal of electron from outer shell
  • results in positive ion=more protons than neutrons
57
Q

what is the first ionisation energy of Na

A

Na(g)= Na+(g) + e-

first ionisation energy of sodium = +494KJmol-1

58
Q

what happens with the ionisation energy when you down a group

A

I.E decreases as the atoms get larger and there is more shielding

59
Q

in group 1, which element has the highest first I.E

A

Li

60
Q

which element has greater shielding-Na or K

A

K- has more shielding

61
Q

what is the test for halide ions

A

add silver nitrate

Chemistry (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions