atoms - the smallest unit of an element each element is made up of only one type of atom (the...
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Atoms
- the smallest unit of an element
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Each element is made up of only one type of atom (the element Carbon is only made up of carbon atoms).
Atoms are so small they cannot be seen with a microscope.
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• The nucleus contains two types of particles: protons and neutrons.
Structure of the Atom
• The center of the atom is called the nucleus.
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Structure of the Atom
• Protons have a positive charge (+).
++• Neutrons have no charge. They are neutral.
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Structure of the Atom, cont’d• Electrons are
always moving or spinning around the nucleus, like planets orbiting the sun.
• The space where the electrons orbit is called the electron cloud.
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Structure of the Atom, cont’d• Electrons have a
negative (-) charge.
• Electrons are much smaller than protons.
–
–
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• The number of protons in an atom equals the number of electrons in an atom. Therefore an atom is electrically neutral.
# protons = # electrons
• What makes atoms different from one another is the number of protons, neutrons and electrons that they have.
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1. Label the picture of an atom using the following codes:
P – Proton
N – Neutron
E - Electrons
2. Color the protons blue.
3. Color the neutrons red.
4. Color the electrons brown.
5. Write the charges beside each one.
Structure of an Atom
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1. Label the picture of an atom using the following codes:
P – Proton
N – Neutron
E - Electrons
2. Color the protons blue.
3. Color the neutrons red.
4. Color the electrons brown.
5. Write the charges beside each one.
PP N
N
E
E
–
–
+
+ o
o
Structure of an Atom
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Atomic Number & Atomic Mass
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12.0116
Ccarbon
• The periodic table includes each element’s:– atomic number
– atomic mass
– symbol
– name
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Atomic Number
• The atomic number is the number of protons an element has.
• The periodic table lists elements in order by their atomic number.
• Remember, the number of protons is the same as the number of electrons.
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Atomic Mass
• The atomic mass (also called mass number) is the weight of one atom of the element.
• Atomic mass will also give you the average number of neutrons in the nucleus by the following formula:
# protons + # neutrons = atomic mass
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• What is the atomic number? 9
9
9
19
10
• How many protons?
• How many electrons?
• What is the atomic mass?
• How many neutrons?
19.009
Ffluorine
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Isotopes
• All atoms of a certain element will always contain the same number of protons, however the number of neutrons can vary.
• Isotopes are atoms that have the same number of protons, but different numbers of neutrons.
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Isotopes
• Carbon-12 has 6 protons and 6 neutrons. Carbon-14 has 6 protons and 8 neutrons.
• The atomic mass is an average of the isotopes so is not always a whole number.
• Isotopes are useful in determining age of fossils, diets of animals, and origins of wood.
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Atomic Mass
• Scientists have chosen the most common isotope of carbon (carbon-12) as a reference.
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• An atom of carbon-12 is assigned a mass of 12 atomic mass units (amu).
• The masses of all other atoms are compared with this mass.
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• One atomic mass unit is 1/12 the mass of a carbon-12 atom.
• The mass of an atom expressed in atomic mass units is called its atomic mass.
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• The atomic mass of an element found in the periodic table is actually calculated from the masses of the element’s isotopes.
• It is a weighted average of the masses of the isotopes – you must take into consideration the percent abundance of each element.
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• Example:
• There are two isotopes for lithium: lithium-6 makes up 7.4% of all lithium atoms and lithium-7 makes up the other 92.6%.
• Calculate the average atomic mass.
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• SOLUTION:
(6amu x 0.074) + (7amu x 0.926) = 0.44 + 6.482
= 6.922 = 6.9amu
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Now it’s your turn……