NAME: ______Chemistry 313 Chapter 4 and 5 CHAPTER 4: FORMATION OF COMPOUNDS Chapter Outline 4.1 The Variety of Compounds Objectives - Distinguish the properties of compounds from those of the elements of which they are composed. - Compare and contrast the properties of sodium chloride, water, and carbon dioxide. - Analyze evidence to conclude that differences exist in the ways compounds form. 4.2 How Elements Form Compounds Vocabulary octet rule noble gas configuration ion ionic compound ionic bond crystal covalent bond covalent compound molecule electrolyte interparticle force Objectives - Model two types of compound formation: ionic and covalent at the atomic level. - Demonstrate how and why atoms achieve chemical stability by bonding. - Compare, using examples, the effect of covalent and ionic bonding on the physical properties of compounds.
CHAPTER 5: TYPES OF COMPOUNDS Chapter Outline 5.1 Ionic Compounds Vocabulary binary compound formula unit oxidation number polyatomic ion
Objectives - Apply ionic charges to writing formulas for ionic compounds. - Apply formulas to name ionic compounds. - Interpret the information in a chemical formula. 5.2 Molecular Substances Vocabulary molecular substance
Objectives - Compare the properties of molecular and ionic substances. - Distinguish among allotropes of an element. - Apply formulas to name molecular compounds. Chemistry 313 Chapter 4
FORMATION OF COMPOUNDS The Variety of Compounds
Slide 2: Sodium Chloride (NaCl) - The chemical name tells you what elements make up the compound: ______and______- Where is it found? o ______
- How is it used? o ______
______
Slide 3: Physical and Chemical Properties of Salt - What are some of the physical properties of NaCl? o It is a white, ______, ______at room temperature
o it is ______
o Melts at ______
o it ______in water
o It only conducts electricity in ______form (dissolved in water) or when melted.
it ______conduct electricity as a solid (but it it ______in water (this makes a great conductor of electricity).
- What are the chemical properties of sal tNaCl? o It does not readily react readily with other substances. ( ______) o Pale green, poisonous gas with choking o Shiny, silvery-white, soft, and odor, and nonmetallic - Slide 4: How do the properties of salt compare with the properties of its component metallic solid o Kills living cells and slightly soluble in elements, sodium and chlorine? o Melt to become liquid at 98°C water o Stored in oil because it reacts with o Used as a disinfectant - ______oxygen and water vapor in air o- ______Condenses into a liquid at -34°C o One of the most reactive of the o One of the most reactive elements common elements o Has industrial importance o Always found combined with other elements. Slide 5: Carbon dioxide (CO2) - The chemical name tells you what elements make up the compound: ______and______- Where is it found? o ______
o ______
- How is it used? o ______
______
Slide 6: Physical and Chemical Properties of Carbon Dioxide - What are some physical properties of CO2? o It is a ______, ______, and ______gas. o Below ______, the gas changes directly to a ______, without first
first becoming a ______( ______) o It is ______in water, but a ______conductor of electricity.
- What are some chemical properties of CO2? - Can you think of any chemical properties of carbon dioxide? o It is relatively______o It is used in ______because it does not support burning.
o It is involved in ______. Slide 7: Properties of Carbon Dioxide - ______-______o Nonmetallic and unreactive at room o Nonmetallic, colorless, odorless, and temperature tasteless gas o Reacts with other elements at high o Oxygen supports burning temperatures o Becomes a liquid when cooled to -183°C o Carbon burns easily and is a good source o Slightly soluble in water of heat o More reactive than carbon and combines o Form a huge variety of compounds (organic with many other elements chemistry) o Most abundant element in Earth’s crust
Slide 8: Dihydrogen monoxide (H2O) - The chemical name tells you what elements make up the compound:
______and______
- Where is it found? o It is approximately ______of Earth’s surface
o Its about ______of the mass of the average human body
- How is it used? o ______
______
Slide 9: Physical and Chemical Properties of Water o What are the physical properties of water? o It is the only one of the three compounds that occurs in Earth’s environment in all ______
o It turns into a gas at ______and turns into a solid at ______
o Pure water ______conduct electricity as a solid, liquid, or a gas.
o It is called the ______because it is good at dissolving other substance. o It is important in the transport of materials.
Slide 10: Chemical Properties of Water What are the chemical properties of water?
o Water is a ______compound that doesn’t break down under normal conditions and doesn’t react with many other substances o It acts as a medium for ______to occur
o It is important during ______o Slide 11: The Properties of Hydrogen and Oxygen
o ______- ______o Nonmetallic, colorless, odorless, and o Lightest and most abundant element in the universe tasteless gas o Nonmetallic, odorless, tasteless, and colorless gas o Oxygen supports burning o Reactive element, so rarely found as a free element o Becomes a liquid when cooled to o Turns into a liquid at -253°C -183°C o Does not conduct electricity o Slightly soluble in water o Slightly soluble in water o More reactive than carbon and combines with many other elements o Most abundant element in Earth’s
Slide 12: Conclusions o Can you make any conclusions about compounds and the elements that make them up? o ______
______
Slide 13: How Elements Form Compounds
o For elements to______, atoms of the elements must ______.
o It is the ______of colliding atoms that interact to form compounds.
◦ Remember from chapter 3 that the properties of elements ______because the number of
______repeat in each group.
◦ The number of valence electrons determines the ______of an atom.
Slide 14: The Octet Rule
o Why are noble gases so unreactive and so stable? ◦ Each noble gas (______) has ______valence electrons
o The ______states that atoms can become______by having ______electrons in their outer energy level.
◦ Elements become more stable by achieving a ______.
◦ They do this by ______, ______or______electrons with other elements.
Slide 15: Electrons can be Transferred o How many valence electrons do sodium and chlorine have?
◦ Sodium has_____ and chlorine has______
o How can both sodium and chlorine achieve a full octet?
o The ______valence electron of ______is transferred to the ______atom.
Slide 16: Ions o When sodium transfers its one valence electron to chlorine both atoms become charged particles called
______
o Metals (like sodium) ______electrons and become ______charged
Particles called ______.
o Non-metals (like chlorine) ______electrons and become ______charged particles called______.
o The strong attractive force between ions of opposite charge creates an ______.
◦ A compound that is composed of ions is called an ______.
Slide 17: Ionic Compounds
Structure Formula - Every positive sodium atom attracts every The ______of a compound tells what negative chlorine atom and vice versa. elements make up the compound and how : o The ions organize themselves into a many ______of each element are definite ______-shaped present in one unit of the compound. arrangement called a ______Sodium chloride = NaCl ____sodium atom and____ chlorine atom o A crystal is a ______make up one unit of ______o ______of atoms, ions or molecules.
Slide 18: Electrons can be shared o When atoms collide with enough energy to react, but neither attracts electrons strongly enough to take electrons from the other atom, the atoms combine by sharing valence electrons. o Electrons can only be shared to form molecules when ______.
o NOTE: Compounds cannot be formed from two ______!!!!!!.
Slide 19: Forming Covalent Compounds o The attraction of two atoms for a shared pair of electrons is called a ______
o A compound whose atoms are held together by covalent bonds is a ______
(also called ______) o A ______is an uncharged group of two or more ______atoms held together by covalent bonds.
o ______covalent bonds are possible when 1, 2 or 3 pairs of electrons are shared.
Slide 20: Ionic vs. Covalent Compounds
______
o Well-organized, tightly bound o Attractive forces between molecules electrons are weak o Form crystals o The forces between particles that o Hard, rough, and brittle make up a substance are called o High melting point interparticle forces o Soluble in water o Liquids or gases at room temperature o Conduct electricity when dissolved o Do not conduct electricity in water o Do not dissolve in water o Any compound that conducts electricity when melted or dissolved in water is an electrolyte.
NAME: ______Chemistry 313 Chapter 4
HOMEWORK #1 1. How do the properties of elements that make up a compound compare to the properties of that compound. Use NaCl (salt) as an example. 2. Classify the following substances as elements or compounds and if they are composed of metals, nonmetals or both.
Substance Element Compound Metal Nonmetal NaCl X X X Sulfur Chlorine gas Carbon dioxide
3. The compounds NaCl, H2O, and CO2 were discussed in section 4.1. For each of the following descriptions, tell which compound fits best.
a. Makes up 70% of Earth’s surface ______b. Important in forming solutions ______c. Formed from a metal and a nonmetal ______d. A dense gas at room temperature ______e. Can commonly be found in all three states of matter ______f. Given off when charcoal burns ______g. Composed of brittle crystals ______
HOMEWORK #2 1. Explain why sodium chloride is a neutral compound even though it is made up of ions that have positive and negative charges.
2. Potassium metal will react with sulfur to form an ionic compound. Use the periodic table to determine the number of valence electrons for each element. Write an ionic equation to show how they would combine to form ions that result in a neutral compound.
3. Why does sodium chloride have to be heated to 800°C before melting?
HOMEWORK #3 1. Compare the formation of H2O from hydrogen and oxygen with the formation of CO2 from carbon and oxygen. In what ways are they similar? In what ways do they differ?
2. What is the octet rule and how does the formation of covalent bonds help to satisfy the octet rule?
3. Draw the Lewis structure for O2 Ionic Compounds
Ionic compounds form from the combination of ______and ______.
Atoms that lose electrons are called ______and have a ______charge.
Atoms that gain electrons are called ______and have a ______charge.
Naming ionic compounds with metals that only form one ion
1. State the name of the first atom 2. Drop the last syllable (or 2) from the second atom name and add –ide
Element Name Element Name
C Carbide S Sulfide
N Nitride Cl Chloride
O Oxide Se Selenide
F Fluoride Br Bromide
P Phosphide I Iodide
Name the following ionic compounds
Compound Compound Name
CaBr2 Calcium Bromide
Na2O
Ag2S
K3P
Al2N3
Given the compound name, identify the ions involved and provide the chemical formula Compound Name Cation Anion Compound
2+ - Beryllium Chloride Be Cl BeCl2
Sodium Sulfide
Lithium Phosphide
Magnesium Nitride
Calcium Oxide
Naming Ionic Compounds Using the Stock System (for atoms that have more than one possible charge) Element 1+ 2+ 3+ 4+
Copper (Cu) X X
Chromium (Cr) X X
Iron (Fe) X X
Lead (Pb) X X
Tin (Sn) X X
Follow the 1st atom name by the Roman numeral that represents its charge in parenthesis
Example Copper (I) Chloride = CuCl or Copper (II) Chloride = CuCl2
Name the following ionic compounds using the stock system
Compound Cation Anion Name
2+ - FeCl2 Fe Cl Iron (II) Chloride
PbF4
Sn3P2
CoO
CrP
Provide the chemical formula give the names of the following ionic compounds
Name Cation Anion Compound 2+ 3- Copper (II) Nitride Cu N Cu3N2
Tin (IV) Oxide
Lead (II) Iodide
Chromium (III) Phosphide
Iron (III) Bromide
Ionic compounds that contain polyatomic cations or anions
+ There is only one polyatomic cation, NH4 (ammonium ion)
When naming polyatomic anions, the charge for each member of a pair is the same. The ions differ by the number of atoms each member contains.
2- 2- Example: SO3 and SO4
The name of the member of the pair with the fewer number of atoms ends in –ite, the other ends in –ate.
2- 2- SO3 (sulfite) and SO4 (Sulfate)
When forming compounds with polyatomic ions, place parenthesis around the entire ion before attempting to add subscripts (balance the charges)
Provide the names of the following compounds which contain polyatomic ions
Compound Cation Anion Name
2+ 3- Ba(NO3)2 Ba NO Barium Nitrate Form the
MgSO3
(NH4)3P
NaNO3
Pb3(PO4)2
compound containing polyatomic ions given the names Name Cation Anion Compound
2+ 3- Magnesium Phosphate Mg PO4 Mg3(PO4)2
Ammonium Sulfite
Calcium Hydroxide
Lithium Nitrate
Aluminum Sulfate
Molecular Compounds
When naming binary molecular compounds, always name the more ______atom first.
Naming Rules
1. If there is more than one of the 1st atom, precede the atom name by the appropriate prefix (di, tri, tetra, penta, hexa, hepta, octa, nona, deca)
Example: C6O2 hexacarbon dioxide
2. If there is only one of the first atom, do not precede the atom name by mono.
CO2 = monocarbon dioxide CO2 = carbon dioxide
3. Precede the second atom name by the appropriate prefix, including mono if there is only one of that atom. Drop the last syllable (or 2) and add –ide to the element name
C2O Dicarbon monoxide
Element Name Element Name
C Carbide S Sulfide
N Nitride Cl Chloride
O Oxide Se Selenide
F Fluoride Br Bromide
P Phosphide I Iodide
Provide the name of the following molecular compounds Compound Compound Name
P6O3 Hexaphosphorus trioxide
NS4
Se8O
C7Br5
S2F2
Provide the Chemical Formulas given the following names
Compound Name Compound
Dinitrogen monofluoride
Nonaphosphorus decachloride
Sulfur hexabromide
Tetracarbon pentasulfide
Octanitrogen trifluoride