Relative isotopic, atomic and molecular mass

Question 1

why do we use relative mass

Answer 1

atoms are so small that they are inconvenient to work with and cannot be measured using any balances in the lab

Question 2

what is the standard

Answer 2

carbon 12, which is assigned exactly 12 mass units

Question 3

RIM

Answer 3

relative isotopic mass

Question 4

relative isotopic abudance

Answer 4

the percentage of an isotope in its natural environment

Question 5

mass spectrometer

Answer 5

used to identify the existence of isotopes and their isotopic abudances, from this data relative atomic masses can be determined

Question 6

how is a mass spectrometer read

Answer 6

the position of each peak represnts an isotope and the height of the peak indicates the isotope abundance

Question 7

symbol for relative atomic mass

Answer 7

Ar

Question 8

relative atomic mass

Answer 8

the relative mass of an element based on the abudances of each isotope

Question 9

formula to calculate relative atomic mass through known relative isotopes and their abundances

Answer 9

Ar = (relative isotopic mass X % abudance) + (relative isotopic mass X % abudance) / 100

Question 10

RMM

Answer 10

relative molecular mass

Question 11

relative molecular mass

Answer 11

mass of one molecule relative to the mass of the c12 atom, is equal to the sum of the relative atomic masses in the molecule

Question 12

relative molecular mass symbol

Answer 12

M/Mr

Question 13

what is the equivalent of molecular mass in ionic compounds

Answer 13

relative formula mass, which is calculated the same way

Question 14

what is percentage composition

Answer 14

tells you the proportion by mass of different elements in a compound

Question 15

how to calculate percentage composition

Answer 15

% of an element in a compound = mass of element in 1 mol of the compound / molecular mass of compound X 100

Question 16

symbol for the mole

Answer 16

n