Unit 5: Diversity of Matter
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2 20 Table of Contents Unit 5: Diversity of Matter Chapter 20: Chemical Bonds 20.1: Stability in Bonding 20.2: Types of Bonds 20.3: Writing Formulas and Naming Compounds
3 20.1 Compounds Stability in Bonding Most matter around you are compounds. Some of the matter around you is in the form of uncombined elements such as copper, sulfur, and oxygen. Like many other sets of elements, these three elements unite chemically to form a compound when the conditions are right.
4 20.1 Compounds Stability in Bonding
5 20.1 Stability in Bonding New Properties
6 20.1 Formulas Stability in Bonding chemical formula- tells what elements a compound contains and the exact number of the atoms of each element.
7 20.1 Stability in Bonding
8 20.1 Stability in Bonding The Unique Noble Gases To understand the stability of the noble gases, it is helpful to look at electron dot diagrams. Electron dot diagrams show only the electrons in the outer energy level of an atom.
9 20.1 Stability in Bonding Energy Levels and Other Elements It is more stable when it is part of a compound.
10 20.1 Stability in Bonding Energy Levels and Other Elements Helium rarely forms compounds but, by itself, the element is a commonly used gas.
11 20.1 Stability in Bonding Energy Levels and Other Elements
12 20.1 Stability in Bonding Outer Levels Getting Their Fill How does hydrogen, or any other element, trying to become stable, gain or lose its outer electrons? Elements become stable by combining with other atoms that also have partially complete outer energy levels. As a result, each achieves stability.
13 20.1 Outer Levels Getting Their Fill Draw This Picture Stability in Bonding
14 20.1 Stability in Bonding Stability Is Reached When atoms gain, lose, or share electrons, a chemical bond forms creating a compound. chemical bond is the force that holds atoms together in a compound.
15 20.1 Section Check Question 1 What tells the elements a compound contains and how many atoms of each element per molecule of the compound?
16 20.1 Section Check Answer A chemical formula is a form of chemical shorthand that tells what elements and how many atoms of each are in one molecule of a compound.
17 20.1 Section Check Question 2 The number of in each group s outer energy level increases across the periodic table. A. electrons B. neutrons C. protons D. protons and neutrons
18 20.1 Section Check Answer The answer is A. Protons and neutrons are located in the nucleus of the atom.
19 20.1 Section Check Question 3 What is the force that holds atoms together in compounds? Answer The force that holds atoms together in compounds is a chemical bond.
20 20.2 Types of Bonds Gain or Loss of Electrons Atoms lose or gain to meet a standard a stable energy level. An atom that has lost or gained electrons is called an ion. Ion- is a charged particle because it now has either more or fewer electrons than protons.
21 20.2 Types of Bonds Gain or Loss of Electrons The positive and negative charges are not balanced. The electric forces between oppositely charged particles hold those compounds together.
22 20.2 Types of Bonds Gain or Loss of Electrons
23 20.2 Types of Bonds A Bond Forms
24 20.2 Types of Bonds The Ionic Bond ionic bond- attraction between the opposite charges of the ions a transfer of electrons takes place. Oxidation Number- Number of electrons a element needs to gain or loose to become stable Looses Electrons = positive Gains Electrons = negative
25 20.2 Types of Bonds The Ionic Bond
26 20.2 Types of Bonds Zero Net Charge Ionic bonds usually are formed by bonding between metals and nonmetals.
27 20.2 Types of Bonds Sharing Electrons Some atoms of nonmetals are unlikely to lose or gain electrons. For example, the elements in Group 4 of the periodic table have four electrons in their outer levels. They would have to either gain or lose four electrons in order to have a stable outer level.
28 20.2 Types of Bonds Sharing Electrons covalent bond Bond between atoms when they share electrons Examples:
29 20.2 Types of Bonds Multiple Bonds A covalent bond also can contain more than one pair of electrons. An example of this is the bond in nitrogen (N 2 ). Each pair of electrons represents a bond.
30 20.2 Types of Bonds Unequal Sharing Electrons are not always shared equally between atoms in a covalent bond. These elements are close together in the upper right-hand corner of the periodic table. The strength of the attraction of each atom to its electrons is related to the size of the atom, the charge of the nucleus, and the total number of electrons the atom contains.
31 20.2 Types of Bonds Unequal Sharing Part of the strength of attraction has to do with how far away from the nucleus the electron being shared is. The other part of the strength of attraction has to do with the size of the positive charge in the nucleus.
32 20.2 Types of Bonds Unequal Sharing One example of this unequal sharing is found in a molecule of hydrogen chloride, HCl. Click image to view movie Chlorine atoms have a stronger attraction for electrons than hydrogen atoms do.
33 20.2 Types of Bonds Unequal Sharing As a result, the electrons shared in hydrogen chloride will spend more time near the chlorine atom than near the hydrogen atom.
34 20.2 Tug-of-War Types of Bonds You might think of the bond as the rope in a tug-of-war, and the shared electrons as the knot in the center of the rope. Each atom in the molecule attracts the electrons that they share. However, sometimes the atoms aren t the same size.
35 20.2 Types of Bonds Polar or Nonpolar? The charge is balanced but not equally distributed. This type of molecule is called polar. polar molecule- is one that has a slightly positive end and a slightly negative end although the overall molecule is neutral.
36 20.2 Types of Bonds Polar or Nonpolar? A nonpolar molecule is one in which electrons are shared equally in bonds. Such a molecule does not have oppositely charged ends. Draw out CCl 4.
37 20.2 Section Check Question 1 When ionic bonds form, the resulting compounds are. A. electrically neutral B. electrically unstable C. negatively charged D. positively charged
38 20.2 Section Check Answer The answer is A. In an ionic bond, a transfer of electrons takes place and the overall neutral charge is maintained.
39 20.2 Section Check Question 2 The attraction that forms between atoms when they share electrons is. A. a binary compound B. a covalent bond C. an ionic bond D. the oxidation number
40 20.2 Section Check Answer The answer is B. A single covalent bond is made up of two shared electrons.
41 20.2 Section Check Question 3 In what type of molecule are electrons shared equally? A. diatomic B. nonpolar C. polar D. water
42 20.2 Section Check Answer The answer is B. In a nonpolar molecule, electrons are shared equally and the molecule does not have oppositely charged ends.
43 20.3 Writing Formulas and Naming Compounds Binary Ionic Compounds A binary compound is one that is composed of two elements. Examples?
44 20.3 Writing Formulas and Naming Compounds Binary Ionic Compounds You need to know which elements are involved and what number of electrons they lose, gain, or share in order to become stable. oxidation number- Number of electrons it gains or loses during a reaction to become stable Where can we find this Info?
45 20.3 Writing Formulas and Naming Compounds Binary Ionic Compounds For ionic compounds the oxidation number is the same as the charge on the ion. For example, a sodium ion has a charge of 1+ and an oxidation number of 1+.
46 20.3 Page 616 Writing Formulas and Naming Compounds Oxidation Numbers
47 20.3 Writing Formulas and Naming Compounds Compounds Are Neutral When writing formulas it is important to remember that although the individual ions in a compound carry charges, the compound itself is neutral. Examples? A formula or compound must have equal positive ions and negative ions so the charges balance. (Example Na+1 Cl 1)
48 20.3 Writing Formulas and Naming Compounds Compounds Are Neutral What if you have a compound like calcium fluoride? **Do example on Paper** A calcium ion has a charge of 2+ and a fluoride ion has a charge of 1. In this case you need to have two fluoride ions for every calcium ion in order for the charges to cancel and the compound to be neutral with the formula CaF 2.
49 20.3 Writing Formulas and Naming Compounds Writing Formulas Formula Writing Rules: 1. Write the symbol of the element that has the positive charge.
50 20.3 Writing Formulas and Naming Compounds Writing Formulas 2. Write the symbol of the element with the negative charge. 3. Switch charges with subscripts - Example
51 20.3 Writing Formulas and Naming Compounds Writing Names Compound naming rules: 1. Write the name of the positive ion.
52 20.3 Writing Formulas and Naming Compounds Writing Names 3. Write the root name of the negative ion. The root is the first part of the element s name. 4. Add the ending - ide to the root.
53 20.3 Writing Formulas and Naming Compounds Writing Names Subscripts do not become part of the name for ionic compounds. However, subscripts can be used to help determine the charges of these metals that have more than one positive charge
54 20.3 Writing Formulas and Naming Compounds Compounds with Complex Ions Not all compounds are binary. Baking soda has the formula NaHCO 3. This is an example of an ionic compound that is not binary.
55 20.3 Writing Formulas and Naming Compounds Compounds with Complex Ions Some compounds, including baking soda, are composed of more than two elements. They contain polyatomic ions.
56 20.3 Writing Formulas and Naming Compounds Compounds with Complex Ions polyatomic ion- a positively or negatively charged group of atoms. So the polyatomic ions as a whole contains two or more elements.
57 20.3 Writing Formulas and Naming Compounds Writing Names The table lists several polyatomic ions. Write the positive ion Then write the name of the negative ion. Examples?
58 20.3 Writing Formulas and Naming Compounds Writing Formulas To write formulas for these compounds, follow the rules for binary compounds, with one addition. When more than one polyatomic ion is needed, write parentheses around the polyatomic ion before adding the subscript.
59 20.3 Writing Formulas and Naming Compounds Naming Binary Covalent Compounds Covalent compounds are those formed between elements that are nonmetals. Some pairs of nonmetals can form more than one compound with each other. Examples: NO, NO2, N2O5, N2O
60 20.3 Writing Formulas and Naming Compounds Using Prefixes Use Prefixes only with covalent bonds Examples: NO NO2 N2O5 N2O
61 20.3 Section Check Question 1 What does the oxidation number of an element tell you? Answer The oxidation number indicates how many electrons an atom has gained, lost, or shared in order to become stable.
62 20.3 Section Check Question 2 A is a compound composed of two elements. Answer A binary compound is composed of two elements. Potassium iodide is a binary ionic compound.
63 20.3 Section Check Question 3 What is a hydrate? Answer A hydrate is a compound that has water chemically attached to its ions. Water is also written into its chemical formula.
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65 End of Chapter Summary File
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lost, gained or shared chemical bonds symbols subscripts NaCl, H O, CaCO, CO
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