Chemical Structure: Structure of Matter. Elements, Ions & Isotopes
Isotopes and Ions VARIATIONS ON THE ATOM. Ions! ITS ABOUT PROTONS AND ELECTRONS.
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Transcript of Isotopes and Ions VARIATIONS ON THE ATOM. Ions! ITS ABOUT PROTONS AND ELECTRONS.
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Isotopes and IonsVARIATIONS ON THE ATOM
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Ions!ITS ABOUT PROTONS AND ELECTRONS
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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 in Water Solution
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Using the Periodic Table
Elements in the Main Groups (A), form fairly consistent ions – LEARN TO USE THE CHART
Group IA will form +1 ions; Group 2A form up to +2; Group 3A form up to +3 ions
Group 4A will form either up to -4 or +4 ions Group 5A will form up to -3 ions; Group 6A up to -2; Group 7A form -1; and Group 8A will not form ions at all
Those elements in the B groups vary and we’ll learn those later
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IsotopesITS ABOUT PROTONS AND NEUTRONS
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Isotopes
•are atoms of the same element that have different mass numbers.
•have the same number of protons, but different numbers of neutrons.
Isotopes
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Atomic SymbolAn atomic symbol
•represents a particular atom of an element.
•gives the mass number in the upper left corner and the atomic number in the lower left corner.
Example: An atom of sodium with atomic number 11 and a mass number 23 has the following atomic symbol:
mass number 23 Na
atomic number 11
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Information from Atomic Symbols
The atomic symbol for a specific atom of an element
gives the
• number of protons (p+),
• number of neutrons (n),
• and number of electrons (e-).
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Information from Atomic Symbols
Examples of number of subatomic particles for atoms
Atomic symbol
16 31 65
O P Zn 8 15 30
8 p+ 15 p+ 30 p+
8 n 16 n 35 n 8 e- 15 e- 30 e-
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Learning Check
Naturally occurring carbon consists of three isotopes: 12C, 13C, and 14C. State the number of protons, neutrons, and electrons in each of the following:
12C 13C 14C 6 6 6
protons ______ ______ ______
neutrons ______ ______ ______
electrons ______ ______ ______
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12C 13C 14C 6 6 6
protons 6 p+ 6 p+ 6 p+
neutrons 6 n 7 n 8 n
electrons 6 e- 6 e- 6 e-
Solution
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Write the atomic symbols for atoms with the following subatomic particles:
A. 8 p+, 8 n, 8 e- ___________
B. 17p+, 20n, 17e- ___________
C. 47p+, 60 n, 47 e- ___________
Learning Check
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A. 8 p+, 8 n, 8 e- 16O
8
B. 17p+, 20 n, 17e- 37Cl 17
C. 47p+, 60 n, 47 e- 107Ag 47
Solution
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Learning Check1. Which of the pairs are isotopes of the same element?2. In which of the pairs do both atoms have 8 neutrons?
A. 15X 15X 8 7
B. 12X 14X 6 6
C. 15X 16X 7 8
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SolutionB. 12X 14X
6 6
The atomic symbols in “B.” represent isotopes of carbon with 6 protons each, but one has 6 neutrons and the other has 8.
C. 15X 16X
7 8
These isotopes of nitrogen and oxygen have 8 neutrons.
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Isotopes of Magnesium
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Isotopes of Magnesium
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Isotopes of Sulfur
A sample of naturallyoccurring sulfur containsseveral isotopes with thefollowing abundances
Isotope % abundance 32S 95.02 33S 0.75 34S 4.21 36S 0.02
32S, 33S, 34S, 36S16 16 16 16
Copyright © 2009 by Pearson Education, Inc.
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Ions and Isotopes in Review
Stable atom: #p+ = #n0 = #e-
Atomic Mass - #n0 = # p+
Atomic Mass - #p+ = #n0
If charge is 0, then #p+ = #e-
If charge is positive, then #p+ > #e- Cation
If charge is negative, then #p+ < #e- Anion
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Examples: Li-1 has gained an electron, meaning there is one more negative charge than positive ones
◦ It has 3 p+ and 4 e-
Li+1 has lost an electron, meaning there is one more positive charge than negative ones
◦ It has 3 p+ and 2 e-
◦ REMEMBER: The # of p+ DO NOT CHANGE◦ Only the number of n0 (isotope) and e- (ion) change
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Cf-3 has an atomic number of 98◦ This means it has 98 p+
◦ Its atomic mass is 216◦ It has 118 n0, (216 – 98), making it an ion and an isotope!◦ Since it has a -3 charge, the number of e- will be 101; (98 + 3)
◦ Zn+1 has 30 p+ and n0; but due to the +1 charge, it has only 29 e-