ionic bonds (site)
TRANSCRIPT
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Ionic Bonds
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Non-metal elements have a strong hold on their electrons as a result of having a high electron affinity. Instead, they easily gain electrons.
Metal elements have a weak hold on electrons and so are easily able to lose them.
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Draw the Bohr model for the following:
Natural: Na Cl State
Stable: Na Cl State
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Ionic Bonds form between molecules with opposite charges (cations and anions). Electrostatic attraction between positive/negative atoms holds ionic molecules together.
Made up of metal and non-metal atoms. The atoms DO NOT share electrons. Total charge is always 0.
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Electrostatic forces are strong, which gives ionic compounds a high melting temperature. Many form a crystalline structure, with hard/straight breaks.
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Practice
Identify the charge the following atoms would need to be stable:– Na– S– Br– Sr
If you were to combine Sodium and Bromine, what would be the resulting compound?
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Swap & Drop Method for Ionic BondingAn atom’s oxidation state is an atom’s charge when it is a stable ion.
Identify the oxidation state for the following
– H–Mg– B– Al– O– Ne
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Swap & Drop Method for Ionic Bonding
Identify the oxidation state for each atom.
Ca Cl Mg O
Al Cl Al O
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Naming Ionic Compounds
Generally, the name for compounds can be obtained by using the following convention:
Name = [Metal] + [Non-Metal] + ide
What would the name for NaCl?
What would the compound for Calcium Bromide be?
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Naming Ionic Compounds
Some metals are able to form multiple ions.
For example, copper can form Cu+ or Cu+2.
You must say which one in naming:– Using Cu+1 :Cu2O
Copper (I) Oxide– Using Cu+2 :CuO
Copper(II)Oxide
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Question• Manganese (Mn) can form the ions
+2, +3, +4, +6, and +7.
• Determine the formula & name for:– Oxygen molecules and Mn+3 and Mn+7
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Identify and name the resulting ionic compound
• Na + F Al + O
• Al + Cl Mg + Cl
• Cu+ + O
• Cu2+ + O
• Fe+3 + S