Question

2.
Define the following:
a) Relative atomic mass of an element
b) Relative molecular mase of a substance
c) Average atomic mass
d) Gram atomic mage of an element
e) Gram molecular mass of an substance​

Answer 1

Each ion, or atom, has a particular mass; similarly, each mole of a given pure substance also has a definite mass. The mass of one mole of atoms of a pure element in grams is equivalent to the atomic mass of that element in atomic mass units (amu) or in grams per mole (g/mol).

Answer 2

Answer:

Explanation:

a) The relative atomic mass of an element is the average mass of its atoms, compared to 1/12th the mass of a carbon-12 atom. The relative atomic mass, A r, of an element is calculated from: the mass numbers of its isotopes. the abundance of these isotopes.

b) The relative molecular mass/relative formula mass is defined as the sum of all the individual atomic masses of ALL the atoms in the formula (Mr). e.g. for ionic compounds e.g. NaCl = 23 + 35.5 58.5) or molecular mass for covalent elements or compounds

c) The average atomic mass of an element is the sum of the masses of its isotopes, each multiplied by its natural abundance (the decimal associated with percent of atoms of that element that are of a given isotopes

d) Gram atomic mass of an element can be defined as the mass of one mole of atoms of a particular element. It is numerically equivalent to the value of the element's atomic mass unit but has its unit in grams.

e) Gram molecular mass is the mass in grams of one mole of a molecular substance. Gram molecular mass is the same as molar mass. The only difference is that gram molecular mass specifies the mass unit to be used.