Chemistry Review
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| What are some key differences between ionic and covalent compounds? | * Ionic compounds have high melting and boiling points
*Covalent compounds have low melting and boiling points.
*Ionic compounds conduct electricity when melted
*Covalent compounds are poor electrical conductors.
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| Provide an example of an ionic and covalent compound. | * Example of an ionic compound: RbF
* Example of a covalent compound: CO2
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| Are ionic compounds usually solids, liquids or gases? | Solids.
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| What state(s) are most common for covalent compounds? | Gases, liquids, or soft solids.
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| Do ionic compounds have high or low melting/boiling points? Explain why. | High melting/boiling points because many have more atoms in each molecule and most have a stronger force between molecules.
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| Do covalent compounds have high or low melting/boiling points? Explain why. | Low melting/boiling points because they have only a few atoms and the forces between molecules is weak.
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| Classify each of the following as a chemical or physical change: a. Rust forming on a coin? b. Metal reacting with an acid to produce hydrogen gas: c. Making popsicles in the freezer: d. Baking bread e. Chopping wood f. Adding sugar to coffee | a. chemical change
b. chemical change
c. physical change
d. chemical change
e. physical change
f. physical change
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| Name these simple ionic compounds: a. CaCl2 b. K2O c. Sc2S3 d. Li3P | a. Calcium chloride
b. Potassium oxide
c. Scandium sulphide
d. Lithium phosphide
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| Write formulas for these simple ionic compounds: a. Beryllium oxide b. Sodium sulphide c. Magnesium nitride d. Zinc chloride | a. BeO
b. Na2S
c. Mg3N2
d. ZNCl2
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| Name these ionic compounds (containing a multivalent ion) a. FeO b. Ni2S3 c. CrCl2 d. TiSe2 | a. Iron (II) oxide
b. Nickel (III) sulphide
c. Chromium (II) chloride)
d.Titanium (IV) selenide
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| Write formulas for these ionic compounds (containing multivalent ions): a. Cobalt (III) bromide b. Chromium (II) oxide c. Niobium (V) fluoride d. Molybdenum (II) nitride | a. CoBr2
b. CrO
c. NbF5
d. Mo3N2
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| Name these ionic compounds (containing polyatomic ions): a. NH3Cl b. Ca(OH)2 c. K2CO3 d. Mg3(PO4)2 | a. Ammonium chloride
b. Calcium hydroxide
c. Potassium carbonate
d. Magnesium phosphate
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| What is a compound? | A pure substance made of two or more elements that are chemically combined.
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| What is an element? | A pure substance that cannot be broken down into simpler substances (because it is composed of only one kind of atom).
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| What is a covalent compound? | A compound in which two or more atoms combine by sharing electrons. Water (H2O) is an example.
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| What is an ionic substance? | A compound in which oppositely charged ions combine due to mutual attraction. Table salt (NaCl) is an example.
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| What is an ionic lattice? | A repeating pattern of positive and negative ions within an ionic compound.
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| What is a polyatomic ion? | An ion composed of more than one type of atom combined by covalent bonds.
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| What is an exothermic reaction? | A reaction that produces energy usually in the form of light or heat.
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| What is an endothermic reaction? | A reaction that absorbs energy.
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| What is a chemical bond? | A chemical bond is...connections between two or more atoms holding them together.
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| What is a precipitate? | A solid substance that forms in a solution.
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