Atomic Structure
Nucleons
 Particles in the ________________ of atoms
◦ ______________
◦ ______________
 These particles are “________________” together to form the dense ________________ charged
nucleus that was discovered by ________________ experiments
Atomic Number
 Equal the number of ________________ in the ________________ on an ________________
 Seen on the periodic table as a whole number
 The number or ________________ determines the ________________ of the ________________
◦ ______ protons is a carbon atom
 Neutral atom◦ Number of ________________ (positive) = number of ________________ (negative)
Isotope
 Atoms of an ________________ that have ________________ numbers of ________________
 For carbon there are 2 predominate ________________:
◦ 12C at 98.9% abundance
◦ 13C at 1.1% abundance
 The above notation in known as ________________ ________________ notation
 There is also ________________ ________________
◦ ________________ -_____ and ________________ -_____
Isotopes of Hydrogen
 Hydrogen-1
◦ ___ proton and ___ neutrons
 Hydrogen-2
◦ ___ proton and ___ neutron
 Hydrogen-3
◦ ___ proton and ___ neutrons
 What is the nuclear notation for these?
◦
◦
◦
Example Problem #1
 Write the following elements in the opposite notation given.
1. Copper-63

7
2. Li

3. Silver-108

22
4. Ne

Mass number
 Total number of ________________ and ________________ in an atom
 The mass number is always a ________________ number
 Looking at Carbon-12, how many protons and neutrons?
◦ ___ protons and ___ neutrons
 ________________ of ________________ = mass number - ________________
 ________________ are ignored in mass number calculations because they weight 1/2000th of a proton
Example Problem #2
 How many protons and neutrons are in 63Cu?
 How many protons and neutrons are in 39K?
Atomic Mass
 ________________ of the masses of all element’s ________________
 How do we arrive at 12.011 g/mol if ________________ and ________________ each weigh 1 amu?
◦ The average of all of the ________________ of ________________ can be used to calculate the
________________ mass of an element
Calculating Atomic Mass
 Using ________________ we can solve for the ________________ Mass of an element using the
following equation:
 (mass of isotope A)(Percent abundance of A) + (mass of isotope B)(Percent Abundance of B) +…. = Molar Mass
Solving Atomic Mass
 For carbon there are 2 predominate ________________:
◦ 12C at 98.9% abundance
◦ 13C at 1.1% abundance
Molar Mass = 12*0.989 + 13*0.011
Molar Mass = 11.868 + 0.143
Molar Mass = 12.011 g/mol
Example Problem #3
 Isotopes of potassium are:
◦ 39K at 93.26% abundance
◦ 40K at 0.012% abundance
◦ 41K at 6.73% abundance
Practice Problem #1
 Isotopes of Silver are:
◦ 107Ag at 51.839% abundance
◦ 109Ag at 48.161% abundance
Particle
Charge
Practice Problem #2
 Number of protons?
◦
 Number of electrons?
◦
 Number of neutrons?
◦
Mass
Location
Practice Problem #3
 Number of protons?
◦
 Number of electrons?
◦
 Number of neutrons?
◦