do now: if a student’s grade is weighted per the table below, what would their grade be?...
TRANSCRIPT
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Do Now:
If a student’s grade is weighted per the table below, what would their grade be?
Weight AverageTests 50% 80
Classwork 30% 95Homework 20% 85
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YWBAT
• Explain what makes elements and isotopes different from each other and how isotopes of an element differ.
• Calculate the atomic mass of an element.
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Distinguishing Among Atoms
• An atom is the smallest particle of an element that still has the chemical properties of that element.
• But what makes atoms of one element different from another?
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Atomic Number
• Atomic Number: the number of protons in the nucleus of an atom of that element.
It’s like an ID number
for an element
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Atomic Number
• Atoms are electrically neutral so
Protons = Electrons
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Mass Number
• Mass Number: total number of protons and neutrons in an atom
Mass Number = protons + neutrons
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Mass Number
• You can also refer to atoms by using the mass number and the name of the element.
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Atoms
If you know the atomic number and mass number, you can determine the atom’s composition.
# Protons = Atomic Number# Electrons = # Protons# Neutrons = Mass Number – Atomic Number
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Practice
How many protons, neutrons, and electrons are in each of the atoms?
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Isotopes
Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
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Hydrogen has 3 isotopes
The correct way to represent an isotope is to write the chemical name followed by the mass number (protons + neutrons)
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Hydrogen has 3 isotopes
The correct way to represent an isotope is to write the chemical name followed by the mass number (protons + neutrons)
1
1
1
1
1
1
1
0
2
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Isotopes
Just because the number of neutrons is changing does not change which element it is because the atomic number does not change.
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Isotopes
• In nature, most elements occur as a mixture of two or more isotopes.
• Each isotope of an element has a fixed mass and a natural percent abundance.
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Average Atomic Mass
• The mass that is listed on the periodic table is an average atomic mass.
• It is a weighted average of the atomic masses of naturally occurring isotopes.
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Calculating Average Atomic MassChlorine-35 has an amu of 34.9689 with an abundance of 75.771% while Chlorine-37 has an amu of 36.9659 and an abundance of 24.229%What is the average atomic mass of chlorine?
Carbon-12 (12.00 amu) makes up 98.93% of all of the carbon atoms, while carbon-13 (13.003 amu) is about 1.07% abundant. What is the average atomic mass of carbon?
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Calculating Average Atomic Mass
Chlorine-35 has an amu of 34.9689 with an abundance of 75.771% while Chlorine-37 has an amu of 36.9659 and an abundance of 24.229%What is the average atomic mass of chlorine? 35.453Carbon-12 (12.00 amu) makes up 98.93% of all of the carbon atoms, while carbon-13 (13.003 amu) is about 1.07% abundant. What is the average atomic mass of carbon? 12.011
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Review
How are the atoms of one element different from the atoms of another element?
How are isotopes of the same element different?
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Electrons and the Structure of the Atom
• Atoms of the same element have the same number of protons, which is equal to an atom’s atomic number.
• But atoms of the same element can have different numbers of neutrons.
• Atoms of the same element with different numbers of neutrons are isotopes.
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Atomic Mass Units• The actual masses of individual atoms are inconveniently small.• So instead, we compare the relative masses of atoms using a
reference isotope as a standard.• The reference isotope chosen is carbon-12.• The isotope of carbon has been assigned a mass of exactly 12 atomic
mass units.
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Atomic Mass Unit (AMU)
• An atomic mass unit is defined as one-twelfth of the mass of a carbon-12 atom.