Unit 5 Chemical Bonding Study Guide

  1. Each family in the periodic table has its own characteristic properties based upon its number of ______.
  2. The valence electrons are those electrons ______from the nucleus.
  3. In an electron dot diagram of carbon, ______dots should be drawn around the element’s symbol.
  4. Each dot in an electron dot diagram stands for ______.
  5. Atoms are stable when the have ______.
  6. Atoms that are not stable form a ______with other atoms to become more stable.
  7. Atoms can lose, ______or ______electrons to form a chemical bond.
  8. The attraction between a positive ion and a negative ion results in an ______bond.
  9. A ______bond is formed when two atoms share electrons equally.
  10. When an atom has an electric charge it is called an ______.
  11. Electrons involved in bonding between atoms are ______electrons.
  12. What is the greatest number of valence electrons an atom can have? ______(with the exception of ______)
  13. When an atom gains an electron, it becomes a ______ion.
  14. If atoms of a halogen nonmetal (group 17) gain one electron, it will have a ______charge.
  15. When an atom loses an electron, it becomes a ______ion.
  16. If an atom of lithium (Li) loses an electron it will have a ______charge.
  17. Ionic compounds are electrically ______.
  18. If I have 3 magnesium atoms each with a 2+ charge, I must have an equal amount of negatively charged ions to balance out the positive charges, so how many nitrogen atoms would I have in in the ionic compound Magnesium Nitride (Mg3N?).______
  19. Aluminum Chloride is an ionic compound with the chemical formula AlCl3. The subscript “3” indicates there are three ______.
  20. In the chemical formula for an ionic compound, the ______ion is written first.
  21. What is the chemical name for the compound with the formula Na2S? ______
  22. In general, ionic compounds are hard, ______, with______, that ______when dissolved in ______.
  23. A ______is formed when 2 pairs of electrons are shared.
  24. Ionic bonds are formed between ______and nonmetals.
  25. When electrons are ______between two atoms, a covalent bond is formed.
  26. Covalent bonds are formed between ______.
  27. The number covalent bonds that a nonmetal atom can form equals the number electrons needed to make a total of ______.
  28. A molecule is ______.
  29. Molecular (covalent)compounds do not ______and have lower ______and ______points.
  30. Molecular compound have lower melting and boiling points because they are held together by a ______bond compared to ions in ionic compounds.
  31. Molecular compounds do not conduct electricity because they do not ______.
  32. A covalent bond in which electrons are shared equally is called a ______.
  33. An example of a covalent compound that has a ______bond is water.
  34. The attraction between a positive metal ion and the electrons surrounding it is a ______bond.
  35. Properties of a metallic bond include malleability, ______, ______, ______, and high ______of solid metals.
  36. The properties of metallic bonds relate to the ______.
  37. Complete the table.

Type of Bond / How bond forms / Charge on bonded atoms / Example
Ionic Bond / Yes; positive and negative
Polar Covalent Bond / Unequal sharing of electrons
Nonpolar Covalent Bond / No
Metallic Bond
  1. Draw electron dot diagrams

K / O / Mg / Al