Download - Grade 8 atoms
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ATOMSInside Out
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AtomThe smallest particle of an element that retains the
properties of that element.
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BEC
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Changes in State
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Changes in State
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Changes in State
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Large Hadron Collider
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Atom• An atom has three parts:• Proton = positive• Neutron = no charge• Electron = negative• The proton & neutron are
found in the center of the atom, a place called the nucleus.
• The electrons orbit the nucleus.
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Atomic number
• Is the number of protons in the nucleus of the atom of an element
Atomic mass
• The total number of protons and neutrons in the nucleus
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Atomic Weight and Isotopes
• Isotopes• Atoms of the same element that have the
same number of protons, but vary in number of neutrons
• Atomic weight• Close to mass number of most abundant
isotope
• Atomic weight reflects natural isotope variation
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How many protons, electrons, and neutrons are in the following atoms?Atomic number
Atomic mass
Beryllium (Be)
4 9
Neon (Ne)
10 20
Sodium (Na)
11 23
Protons Electrons Neutrons
4 4 5 10 10 10
11 11 12
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Terms
• Isotopes = atoms of a given element that differ in mass number– Isotopes have the same number of
_____________.– Isotopes differ in the number of _______.
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Isotopes
• All atoms of an element have the SAME number of protons (p+)
• The p+ number is the atomic number (Z)– This is a constant– For example: All Sodium (Na) atoms have 11 p+
– If an atom loses a proton, it becomes a different element
• If Na loses 1 p+, then it has become Neon (Ne)
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Z = atomic number = p+
• The number of protons identifies the atom and which element it is
• In a stable atom:– # p+ = # n0 = # e-
– Thus, Na in its stable form has 11 p+; 11 n0; and 11 e-
– If it has an unequal number of p+ and n0, then it is called an ISOTOPE
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• Theoretically – an element can have as many isotopes of itself as it has neutrons, or it can add an unlimited number of n0
• For example: H has 3; C has 16; Al has 25– These can be looked up in the CRC (the
Chemistry/Physics Data Bible) or on the internet– Remember – a change in the number of n0 does
not change the element’s atom – only a change in the number of protons can do that!
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The Carbon Isotope
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Ions• Ions are when an atom has an unequal
number of p+ and e-
• Remember – a stable atom has a neutral overall charge due its equal number of p+ and e-
• When an atom loses or gains an e-, its charge changes accordingly– Loss of e- means a + charge; gaining an e- means a
– charge for the atom
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Losing or Gaining e- . . . . .• If an atom loses an e-, then it has more p+ than
e- and it will have an overall positive charge• Different elements’ atoms can lose 1, 2, 3, or
even 4 electrons depending on various factors• If an atom has LOST e-, then it is called a
CATION or a positive ion– A Cation would be written as Al+ (the one being
understood) or Al+3
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• Atoms can also gain electrons• If an atom gains electrons (from 1 up to 4), then it
will have more e- than p+ and will end up having an overall negative charge
• A negatively charged ion is called an ANION
– The element is shown this like: Na- (the 1 is understood) or Na-2
• The losing or gaining of electrons determines what type of bonds the atoms will form, and which atoms will bond to others
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Ions
• Na atom_____ protons _____ electrons
• Na+ ion _____ protons _____ electrons
Name of ion: sodium ion
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Ions
• Calcium atom_____ protons _____ electrons
• Ca 2+ ion _____ protons _____ electrons
Name of ion: calcium ion
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Ions
• Sulfur atom_____ protons _____ electrons
• S2- ion _____ protons _____ electrons
Name of ion: sulfide ion
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Ion Charge and the Periodic Table
Group # Ion Charge # e- lost/gained
I A 1+ 1 e- lost
II A 2+ 2 e- lost
III A metals 3+ 3 e- lost
V A nonmetals 3- 3 e- gained
VI A nonmetals 2- 2 e- gained
VII A 1- 1 e- gained
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Naming Ions
• Name of a monatomic cation is the name of the element– Examples:
• Ca 2+ calcium ion• Al 3+ aluminum ion• K+
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Naming Ions
• Monatomic anions are named by changing end of the name of the element to “ide”
Example: S2- sulfide ion
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Naming Ions
• You need to know:N3- nitride ionP3- phosphide ionO2- oxide ionS2- sulfide ionF- fluoride ionCl - chloride ionBr- bromide ionI- iodide ion