Mole

• Molar mass is numerically equal with atomic mass (amu).

• Similarly, molar mass of a molecule is numerically equal with its molecular mass.
• The mass in amu of one atom or molecule is molecular mass.

• Atomic theory states that atoms are made of protons and neutrons in the nucleus and electrons outside the nucleus.

• The mass in grams of one mole of a substance is molar mass.
• For ionic compounds, the term molecular mass is inappropriate since they are composed of charged particles or ions. There are NO MOLECULES in ionic compounds.
• Mole represents the number of particles present in exactly 12 grams of carbon-12.

• One mole of something is equal to 6.02x10^23.
• The expanded form of 6.02x10^23 is 602,000,000,000,000,000,000,000.

• We use the unit mole to count the molecules.
• The goal in dimensional analysis is to cancel out units other than the desired units through the use of fixed relationships.

• Fixed relationships can be written in ratio or fraction and is also called as conversion factors.
• Conversion from mass to mole, mole to the number of particles and vice versa can be easily determined using dimensional analysis.
• The amount of matter can be expressed in three different ways: mass in grams, number of particles, and mole.

• The symbol of grams per mole is g/mol.

• The molar mass is the mass equivalent to one mole of a substance.
• The mass in grams of one mole of a substance is called molar mass.

• The unit for molar mass is grams per mole.
• One mole of a substance consists of 6.02x10^23 particles of that substance.

• When carbon burns, one mole of carbon atoms reacts completely with one mole of oxygen molecules.
• The symbol of Dalton is D.

• The molecular mass is simply the sum of the masses of the atoms in the molecule of the substance.
• The atomic mass unit is also known as the unified atomic mass unit and Dalton.

• The symbol is unified atomic mass unit is u.
• One amu is equivalent to 1/12 of the mass of a carbon-12 isotope.

• Like atomic mass, molecular and formula mass are the relative mass of the carbon-12 isotope as standard.
• Helium contains two protons, two neutrons, and two electrons.

• The mass of an atom can be expressed in atomic mass unit.
• Atoms are made up of protons, electrons, and neutrons.

• The mass of the electron is so small that it does not contribute to the mass of the atom.
• One amu is equivalent to 1.66054x10^-24 gram.

• The mass of the proton and neutron is approximately 1 amu.
• Amedeo Avogrado is an Italian scientist.

• The mass can be expressed in atomic mass unit (amu) instead of grams, which is a more convenient way of expressing very small masses.
• The mass of protons is 1.672623x10^-24.

• The mass of neutrons 1.67495x10^-24.
• The mass of an atom depends mainly on the number of protons and neutrons inside the nucleus since the mass of the electron is very small.

• The mass of electrons is 9.1093897x10^-28.
• The development of the atomic theory led to the simple view of the atoms as having protons, electrons, and neutrons.

• The protons and neutrons are in the nucleus, while the electrons are found outside the nucleus.