CHEMICAL BONDS AND CHEMICAL REACTIONS

Chapter 18 Section 1: Stability in Bond

Pg. 552-553

  1. What is a chemical formula?
  2. What does a ‘subscript’ indicate in a chemical formula?

How many atoms total are in sand, SiO2?

Pg. 554-556

  1. Why are the noble gases so “unique”?
  2. Describe why chemical bonding occurs.
  3. Give two examples of how bonds can form.

Chapter 18 Section 2: Types of Bonds

Pg. 558

  1. What is an ion?
  2. What is the difference between an anion and cation?

Pg. 559

  1. Explain the transfer of electrons with the chemical bond, KI, Potassium Iodide

Pg. 560

  1. What is an ionic bond?

*Typically, an ionic bond forms between metals and non-metals

  1. Draw out the figure below between Mg and Cl2

Pg. 561

  1. What is a covalent compound?
  2. Draw out a covalent bond of water using the Lewis dot structure (Figure 10)

Covalent compounds can also contain more than one pair of electrons, these are known as diatomic molecules (molecule- more than one atom, such as H2, N2,)

  1. Draw out an example of a diatomic molecule using the Lewis dot structure

Pg. 562-563 SUMMARY

When electrons are shared in covalent bonds by similar or identical atoms, like N2 or O2, the electron charge is shared equally across the bond, this type of bond is called a nonpolar bond. Similarly, a nonpolar molecule is. A molecule without oppositely charged ends. A nonpolar bond results in a nonpolar molecule.

However, some molecules are not shared equally, and because of this, the charge can be concentrated more on one end than the other. When this happens, you end up with partial charges. This “tug-of-war” that causes unequally shared charges is known as polar, meaning having opposite ends. A polar bond is a bond in which electrons are shared unequally, leaving one end slightly more positive, and another, slightly more negative. A polar molecule is one in which the unequal sharing of electrons results in a slightly positive end and a slightly negative end. A polar bond results in a polar molecule.

WATER IS A POLAR MOLECULE

Challenge

Identify the following compounds as either covalent or ionic

H2O / NaCl / CaO / SOs / MgCl2

CHAPTER 18 Section 3: WRITING FORMULAS

Pg. 565

  1. What is an oxidation number?
  2. What is the common oxidation number for elements in Group 1?
  3. Group 2? Group 13? Group 14? Group 15? Group 16? Group 17? Group 18?

CHAPTER 19. Section 1: CHEMICAL REACTIONS

Pg. 582

  1. What is a chemical reaction?
  2. Explain Antoine Lavoisier’s contribution to science.
  3. What is this also known as?

Label the reactants and the products for the following chemical equation:Na2 + 2Cl  2NaCl

Pg. 584-585

  1. What is a chemical equation?
  2. What are coefficients?
  3. Write out the chemical equation for the equation shown on page 584 with NiCl and NaOH
  4. Label the reactants and products
  5. Underline any coefficients

Pg. 586-587

Read the steps for balancing equations. Once you feel comfortable, try balancing the equations on pg. 587. The practice problems 1 & 2

CHAPTER 19. Section 3 CHEMICAL REACTIONS AND ENERGY

Pg. 595-596

  1. Explain the difference between exothermic and endothermic reactions. Provide examples for each

CHAPTER 19. Section 4 REACTION RATES & EQUILIBRIUM

Pg. 598-599

  1. What is a reaction rate?

Pg. 599-601

  1. Explain the 5 factors that affect reaction rates