Atomic mass unit (amu)
The mass of one singular proton or neutron
Atomic number
The number of protons in an atom (top of element card)
Mass number
The sum of protons and neutrons in an atom combined
Atomic mass
The average mass of an atom based on its abundance of isotopes
- Is = to molar mass
How do you find the atomic mass of an element
∑n(fraction of isotope n that makes up the element) x (amu mass of that isotope n)
How do you read a mass spectrometry graph
x-axis: The position of each peak indicates the mass of the isotope
y-axis: The height of each peak indicates the relative abundance of the isotope
Pure substance vs. mixture
Pure substance = only 1 type of atom or molecule
Mixture = 2 or more pure substances mixed together
Pure element vs. compound
Pure element = A pure substance that cannot be further simplified (individual oxygen and hydrogen atoms)
Compound = A pure substance with only 1 type of molecule (water only contains water molecules made of oxygen and hydrogen)
Heterogeneous vs. homogeneous mixture
Heterogeneous = molecules are distinct from each other
Homogeneous = molecules mix together evenly (dissolving)
What is a mole and what does it measure
- A mole is a measure of amount
- 1 mole of anything has 6.022x1023 units
Molar mass (what is it equal to)
molar mass is the mass (weight) of 1 mole of atoms of a given element
- Molar mass in g = atomic mass
Mole (amount) ⇌ grams (weight)
# of Particles/atoms ⇋ (1 mole ÷ 6.022x1023) ⇋ (molar mass in g ÷ 1 mole) ⇋ mass in g
Law of conservation of mass
The total mass of reactants consumed is = to the total mass of products formed
In isotope notation the ___ is on the bottom, and the ___ is on the top representing the different ___
- atomic number (# of protons)
- Mass number (# of protons and neutrons combined)
- The different number of neutrons that isotopes of the same element can have (This is the only number that changes in standard notation)