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Study Guide:Acids & Bases, Types of Reactions, Balancing Chemical Equations, Bonding& Nomenclature

  1. Matter is not created or destroyed. The mass of the reactants is equal to the mass of the products. This is known as .
  1. The equation A + BC  B + AC represents.
  1. The equation A + B  AB represents.
  1. The equation AB + CD  AD + CB represents.
  1. The equations AB  A + B represents.
  1. The elements or compounds produced by a chemical reaction (the ending materials in a chemical reaction) are called .
  1. The starting materials in a reaction—the elements or compounds that enter into a chemical reaction—are called .
  1. How many total atoms are in the compound Fe2O3?. How manytotal atoms are in S5I7? .

Balance the following equations, and name the type of reaction taking place:

  1. ____Na + ____Cl2____NaCl
  2. The reaction in # 9 is a ______reaction.
  1. _____H2SO4 _____H2 + ___ SO4
  2. The reaction in # 11 is a ______reaction.
  1. ____Fe + ____Ag(NO3)____Fe(NO3)2+____Ag
  2. The reaction in # 13 is a ______reaction.
  1. ____Pb(NO3)2 + ____AlCl3 ____PbCl2 +____Al(NO3)3
  2. The reaction in question # 13 is a ______reaction.
  1. A chemical bond in which one atom loses electron(s) to form a positive ion and the other atoms gains the electron(s) to form a negative ion is called ______.
  2. A chemical bond formed when two atoms share electrons is called______.
  3. Compounds formed between two nonmetals are ______compounds.
  4. Compounds formed between one metal and one nonmetal are ______compounds.
  5. Correctly identify the Lewis dot structures below.
  6. B. C.
  1. How many valence electrons do the alkali metals have? How does the periodic table help you determine this?
  2. How many valence electrons to the alkaline earth metal have? How does the periodic table help you determine this?
  3. How many valence electrons do the halogens have? How does the periodic table help you determine this?
  4. How many valence electrons do the nonmetals in the Nitrogen group have? How does the periodic table help you determine this?
  5. How many atoms of Chlorine are needed to form an ionic compound with Magnesium? How do you know this?
  6. How many atoms of Iodine are needed to form an ionic compound with Strontium? How do you know this?
  7. How many atoms of Bromine are needed to form an ionic compound with Paladium (IV)? How do you know this?
  8. How many atoms of oxygen are needed to form an ionic compound with Manganese (II)? How do you know this?
  9. The prefix ______is used to represent “one”.
  10. The prefix ______is used to represent “two”.
  11. The prefix ______is used to represent “three”.
  12. The prefix ______is used to represent “four”.
  13. The prefix ______is used to represent “five”.
  14. The prefix ______is used to represent “six”.
  15. The prefix ______is used to represent “seven”.
  16. The prefix ______is used to represent “eight”.
  17. The prefix ______is used to represent “nine”.
  18. The prefix ______is used to represent “ten”.
  19. The Roman numeral “II” stands for ______.
  20. The Roman numeral “III” stands for ______.
  21. The Roman numeral “IV” stands for ______.
  22. The Roman numeral “V” stands for ______.
  23. The Roman numeral “VI” stands for ______.
  24. The Roman numeral “VII” stands for ______.
  25. The Roman numeral “VIII” stands for ______.
  26. The Roman numeral “IX” stands for ______.
  27. The Roman numeral “X” stands for ______.
  28. When naming compounds, when do you use prefixes like di, tri and tetra?
  29. When naming compounds, when do you use Roman numbers like (II) , (III) and (IV)?

First state if the compound is ionic or covalent, then name the following compounds:

  1. Ionic or covalent? P2F6 is named ______
  2. Ionic or covalent? Li2O is named ______
  3. Ionic or covalent? SiH4 is named ______
  4. Ionic or covalent? Fe2S3 is named ______

What are the formulas for these compounds? List if the compound is ionic or covalent.

  1. Iron (III) Chloride- the formula is ______and it is ______compound.
  2. Magnesium Oxide-the formula is ______and it is ______compound.
  3. Carbon Triphosphide-the formula is ______and it is ______compound.
  4. TetraaresenicPentafluoride -the formula is ______and it is ______compound.

What are the names of these compounds?

  1. CaF2
  2. BeO
  3. K2O
  4. FeO
  5. CO3
  6. NO
  7. CH4
  8. PF5

What are the formulas for these compounds?

  1. Lithium Phosphide
  2. Copper(III) Chloride
  3. Zinc Oxide
  4. Molybdenum(III) Nitride
  5. Carbon Disulfide
  6. DiaresenicTrifluoride
  7. Silicon Tetraiodide

  1. Which of the molecules shown below would have the strongest bond? Explain your decision.
  2. B. C.
  1. Acids turn pH paper ______while bases turn pH paper ______.
  1. What are three common household acids? ______.
  2. List some characteristics of acids:
  1. What are three common household bases?____.
  2. List some characteristics of bases:
  1. 100g of copper beads were placed in a lidded jar (its mass is 150g). 5g of water was added and the jar was sealed tight. After 30 days, the copper hadcorroded and turned green. Before opening, the jar was placed on a balance scale and its mass was measured. What do you predict the mass was, and why do you predict that mass?
  1. 100g of a yellow powder reacted with 400g of a clear, colorless liquid. A lime green solution was formed and a black precipitate was formed during the reaction. After the reaction stopped, the precipitate was separated from the lime green solution, and it as found to have a mass of 50g. What was the mass of the remaining solution?

82. What is the product of an acid (HCl) reacting with a base (NaOH)? Write the equation & explain what occurs.