Key Terms: Nucleons Atomic Number Isotope Atomic Mass.

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Presentation transcript:

Key Terms: Nucleons Atomic Number Isotope Atomic Mass

 Particles in the nucleus of atoms ◦ Protons ◦ Neutrons  These particles are “bound” together to form the dense positively charged nucleus that was discovered by Rutherford’s experiments

 Equal the number of protons in the nucleus on an atom  Seen on the periodic table as a whole number  The number or protons determines the identity of the element ◦ 6 protons is a carbon atom  Neutral atom- ◦ Number of protons (positive) = number of electrons (negative)

 Atoms of an element that have different numbers of neutrons  For carbon there are 2 predominate isotopes: ◦ 12 C at 98.9% abundance ◦ 13 C at 1.1% abundance  The above notation in known as nuclear symbol notation  There is also hyphen notation ◦ Carbon-12 and Carbon-13

Mass spectrometry is a method for seeing isotopes and their respective ratios (CuI) 3

 Hydrogen-1 ◦ 1 proton and 0 neutrons  Hydrogen-2 ◦ 1 proton and 1 neutron  Hydrogen-3 ◦ 1 proton and 2 neutrons  What is the nuclear notation for these? ◦1H◦1H ◦2H◦2H ◦3H◦3H

 Write the following elements in the opposite notation given. 1.Copper-63  63 Cu 2. 7 Li  Lithium-7 3.Silver-108  108 Ag Ne  Neon-22

 Total number of protons and neutrons in an atom  The mass number is always a whole number  Looking at Carbon-12, how many protons and neutrons? ◦ 6 protons and 6 neutrons  Number of neutrons = mass number - protons  Electrons are ignored in mass number calculations because they weigh 1/2000 th of a proton

 How many protons and neutrons are in 63 Cu? ◦ Atomic number = 29  number of protons ◦ 63 mass number – 29 protons = 34 neutrons  How many protons and neutrons are in 39 K? ◦ Atomic number = 19  number of protons ◦ 39 mass number – 19 protons = 20 neutrons

 Average of the masses of all element’s isotopes  How do we arrive at g/mol if protons and neutrons each weigh 1 amu? ◦ The average of all of the abundances of isotopes can be used to calculate the atomic mass of an element

 Using isotopes we can solve for the Atomic 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

 For carbon there are 2 predominate isotopes: ◦ 12 C at 98.9% abundance ◦ 13 C at 1.1% abundance Molar Mass = 12* *0.011 Molar Mass = Molar Mass = g/mol

 Isotopes of potassium are: ◦ 39 K at 93.26% abundance ◦ 40 K at 0.012% abundance ◦ 41 K at 6.73% abundance Molar Mass = 39* * * Molar Mass = Molar Mass = 39.1 g/mol

 Isotopes of Silver are: ◦ 107 Ag at % abundance ◦ 109 Ag at % abundance Molar Mass = 107* * Molar Mass = Molar Mass =

ParticleChargeMassLocation Proton+11 amuNucleus NeutronNeutral1 amuNucleus Electron0Electron cloud

 Number of protons? ◦ 26  Number of electrons? ◦ 26  Number of neutrons? ◦ 30

 Number of protons? ◦8◦8  Number of electrons? ◦8◦8  Number of neutrons ◦8◦8