Physical Science Test #2 Study Guide
Chemical Bonding - Chapter 19
1. Elements in the same group on the Periodic Table have the same number of _____________ electrons.
2. Metals are found on the ____________ side of the Periodic Table. ______________ are on the right
side. ________________ are found along the zig-zag that separates metals and nonmetals.
3. What ending do we change binary compounds endings to?
4. What is unique about the noble gases?
5. An element is chemically stable when it obtains _______________ valence electrons.
6. Ionic bonds result from atoms ________________ electrons. Ionic bonds are usually formed between
atoms of ______________ and nonmetals.
7. _______________ bonds result from atoms sharing electrons. These bonds are usually formed between
_________________ and nonmetals. If the sharing of the electrons is equal then the bond is
______________ _______________. If the sharing of the electrons is ______________ then it is a
polar covalent bond.
8. Write the chemical formula for the compounds that are made from the following elements. Then name
the compound.
Aluminum and Sulfur
Calcium and Bromine
9. What is the name of this covalent compound? P2F5
10. Explain the difference between ionic and covalent bonds.
11. Complete the following table:
Chemical formula
Name
P5O3
Magnesium Nitride
heptanitrogen hexafluoride
Type of compound (ionic
or covalent)
Chemical Reactions – Chapter 20
12. When balancing chemical equations, you are only allowed to adjust the ________________.
13. Name and describe the 4 types of chemical reactions.
14. Balance and classify the following chemical reactions.
__CuO + ___Al
___Al2O3 + ___Cu
___Cl2 + ___NaBr →
___NaCl + ___Br2
___BaCl2 + ___Na2 SO4 →
___N2(g) + ___H2(g) →
___NaCl + ___BaSO4
Type___________________
Type___________________
Type___________________
___NH3(g)
Type__________________
___ Cu2O + _____ C  ____ Cu +____ CO2
Type__________________
_____ Fe + _____ Cl2
Type__________________
_____ FeCl
_____ Na + _____ HCl  _____ NaCl + _____ H2
Type__________________
_____ KCl + _____ NaBr  _____ KBr + _____ NaCl
Type__________________
Solutions – Chapter 22
15. In a solution, the thing being dissolved is the _______________ and the thing doing the dissolving is the
______________________.
16. In saltwater, the solvent is the _____________________.
17. A solution that conducts electricity is an ___________________.
18. List three ways that you can increase the solubility of a solid in a liquid.
19. Explain the differences between unsaturated, saturated, and supersaturated solutions.
20. Compare a dilute and a concentrated solution.
21. What type of solution do you have if you
dissolve 20 grams of KNO3 into 100 grams of
water at 40 o C?
22. What type of solution do you have if you have
60 grams of NH4Cl into 100 grams of water at
90 o C?
23. What type of solution do you have if you
dissolve 150 grams of KI into 100 grams of
water at 10 o C?
Acids and Bases – Chapter 23
24. A substance that produces hydrogen ions (H+) when dissolved in water is an ________.
25. An _________________ is something that changes color in the presence of an acid or a base.
26. A substance that has a pH = 13 and has a slippery feel, then we can say for sure that substance is a
______________.
27. If an acid only partially dissolves in water, then we can say it is a ________ acid.
28. Name four household acids and four household bases.
29. List common properties of acids and common properties of bases.