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chemistry > MODULE 2 > Flashcards

MODULE 2 Flashcards

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1
Q

Who are the scientist’s involved with discovering the atom

A

Enest rutherford, jj thomson, Dalton, Bohr

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2
Q

charge of portons, neutrons and electrons

A

+1, 0 , -1

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2
Q

How are elememnts oredred in the periodic table

A

by proton number

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3
Q

relative mass

A

1, 1, 1/2000

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4
Q

isotopes

A

atoms of an alement with the same number oif protons but a different number of neutrons

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5
Q

reactions of isotopes

A

dont react differently, as they have the same amount of electrons and that is what makes the chemical reacrtivity differ

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6
Q

why aew ions charged

A

unbalanced numbers of protons and electrons

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7
Q

relative masses

A

comparinf the masses of different atoms

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8
Q

what is carbon-12

A

the international standard for the measurement of reltaive atomic mass

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9
Q

relative isotopoic mass

A

same as mass number

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10
Q

relative atomic mass

A

differebnt abundances and relative masses of the different isotopesd in an atom

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11
Q

calculate rAM

A

add the percentages of the isotopes, add the numbers near the dash, divide the numbers near dash by %. always over 100

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12
Q

MR

A

add together thr reltaive atomic masses of each atom making up a molecule compare to carbon-12

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13
Q

RFM

A

add together RAM of each atom

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14
Q

mass spectrometry

A

identifiese unknown compounds, abundances of isotopes

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15
Q

what does y-axis show abnd the x-axis in a mass spec

A

y-axis= percentage abundance / x-axis=mass/charge ratio

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16
Q

deteremining RAM from mass spec

A

find isotopic masses and relative abundances . the % times the number of isotope over sum of the %

17
Q

mole equation

A

mass=mr *mol

18
Q

mole equation

A

PV=NRT ideal gas constant

19
Q

units for this

A

1 atm. 1m^3. mol. 8.314. 273kelvin

20
Q

other mole equation

A

mol=volume/24 gas at room temp and pressure. at dm3

21
Q

number of molecules equation

A

mol * 6.023*10^23

22
Q

concentration and volume / mol /mass equation

A

mass/volume=conc / mol/volume=conc.

23
Q

% yield equation

A

actual amount of product/ theoretical amount *100

24
Q

atom economy equation

A

molar mass of desired product/sum of molar mass of all products *100

25
Q

what is stoichiometry

A

tells you the number of moles of each species that will react together
and studies amount of substances involed

26
Q

composition by mass

A

given %’s - you have to take the %’s and see them as masses.

27
Q

example: 4.125g of compound D is reacted with an excess of hydrogen chloride. the mixture of products contains 95% by mass of one product and 5% by mass of the other product

A

compound D formula=C7H16O
MR=110
MR of HCL=36.5
mol of D=4.125/110 = 0.036/0.0375
mol of HCL= 0.0375
mass of hcl=36.5*0.0375=1.36875(1.37)
add two masses= 4.125+1.368=5.219
95% of this =5.22g
55 of this=0.27g

28
Q

what is the atom economy if the desired product is the only product!

A

100%

29
Q

common acids need to know

A

HNO3/ H2SO4/ HCL

30
Q

ACID DEFINITION

A

produces H+ ions, left side of PH colour red most

31
Q

common bases

A

NaOH,MG(OH)2, MgO,CuO, NH3

32
Q

DEIFNITION OF BASES

A

produce OH^- ions , right siode of ph blue and purple

33
Q

formation of salts

A

from neutralisation reactions with acids and bases; metal oxides, metal carbonates, metal hydroxides

33
Q
A
34
Q

shown by…

A

a dot, rellative number of water molecules are put after the dot. empirical formula put before dot.

34
Q

Dot formulae

A

showsa the amount of water contained in a compound, gives the ratio between the number of compound molecules and water molecules

35
Q

how can you work out how many water molecules are present

A

use the number of hydrogen atoms. if there are 10 H atoms, there will be 5 water molecules (H2O)

36
Q
A
37
Q
A

chemistry (2 decks)

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