NOTES: 7.1 - Ions. Valence Electrons: ● Knowing electron configurations is important because the...
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Transcript of NOTES: 7.1 - Ions. Valence Electrons: ● Knowing electron configurations is important because the...
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NOTES: 7.1 - Ions
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Valence Electrons:
● Knowing electron configurations is important because the number of valence electrons determines the chemical properties of an element.
● Valence Electrons: The e- in the highest occupied energy level of an element’s atoms.
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Valence Electrons:
● All elements in a particular group or family have the same number of valence electrons (and this number is equal to the group number of that element)
Examples:
● Group 1 elements (Na, K, Li, H): 1 valence e-.
● Group 2 elements (Mg, Ca, Be): 2 valence e-.
● Group 17 (7A) elements (Cl, F, Br): 7 valence e-.
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LEWIS STRUCTURES:
● Electron dot structures show the valence electrons as dots around the element’s symbol:
● Li
● B
● Si
● N
● O
● F
● Ne
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LEWIS STRUCTURES:
● Electron dot structures show the valence electrons as dots around the element’s symbol:
● Li
● B
● Si
● N
● O
● F
● Ne
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Which elements form ionic compounds and which elements form covalent (molecular) compounds??
General Rule of Thumb:
metal + nonmetal = IONIC
metal + polyatomic anion = IONIC
polyatomic cation + anion = IONIC
nonmetal + nonmetal(s) = COVALENT
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Why are ionic compounds so stable?
● IONIC BONDS:
-metal plus a nonmetal
-cations plus anions
-opposite charges attract
● Examples:
Na+ and Cl- form NaCl
Al3+ and Br- form AlBr3
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Ionic Bonds:Isn’t it ionic that opposites attract?
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OCTET RULE:
● Noble gas atoms are very stable; they have stable electron configurations. In forming compounds, atoms make adjustments to achieve the lowest possible (or most stable) energy.
● Octet rule: atoms react by changing the number of electrons so as to acquire the stable electron structure of a noble gas.
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Formation of Cations and Anions
● can be predicted using the octet rule (not always followed, but a good general rule to follow for the representative elements)
-full outer energy level
-eight electrons (s2p6)
**explains formation of both cations and anions
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CATIONS:
● Na: 1s2 2s2 2p6 3s1
● Na+:
● Mg: 1s2 2s2 2p6 3s2
● Mg2+:
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CATIONS:
● Na: 1s2 2s2 2p6 3s1
● Na+: 1s2 2s2 2p6
● Mg: 1s2 2s2 2p6 3s2
● Mg2+: 1s2 2s2 2p6
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OCTET RULE:
● Atoms of METALS obey this rule by losing electrons.
Na:
Na+:
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OCTET RULE:
● Atoms of METALS obey this rule by losing electrons.
Na:
Na+:
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ANIONS:
● Cl: 1s2 2s2 2p6 3s2 3p5
● Cl-:
● O:1s2 2s2 2p4
● O2-:
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ANIONS:
● Cl: 1s2 2s2 2p6 3s2 3p5
● Cl-: 1s2 2s2 2p6 3s2 3p6
● O: 1s2 2s2 2p4
● O2-: 1s2 2s2 2p6
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OCTET RULE:
● Atoms of NONMETALS obey this rule by gaining electrons.
Cl:
Cl-:
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OCTET RULE:
● Atoms of NONMETALS obey this rule by gaining electrons.
Cl:
Cl-:
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OCTET RULE:
● Transition metals are exceptions to this rule.
Example: silver (Ag) Ag+
By losing one electron, it acquires a relatively stable configuration with its 4d sublevel filled (pseudo noble-gas)
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OCTET RULE:
● Transition metals are exceptions to this rule.Example: silver (Ag) Ag+
By losing one electron, it acquires a relatively stable configuration with its 4d sublevel filled (pseudo noble-gas)