UNIT 2 CHAPTER 20 CHEMICAL BONDS OCTOBER 5-9, 12-16, 2015.
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Transcript of UNIT 2 CHAPTER 20 CHEMICAL BONDS OCTOBER 5-9, 12-16, 2015.
![Page 1: UNIT 2 CHAPTER 20 CHEMICAL BONDS OCTOBER 5-9, 12-16, 2015.](https://reader038.fdocuments.in/reader038/viewer/2022103006/56649f1c5503460f94c331e5/html5/thumbnails/1.jpg)
UNIT 2CHAPTER 20
CHEMICAL BONDSOCTOBER 5-9, 12-16, 2015
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DO NOW:
1. Review “Composition of Matter” in your interactive notebook.
2. List 4 compounds that you already know.
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HOMEWORK
DUE Friday, October 9: Science Fair Research Paper, Bibliography
Bring your textbook Wednesday!!
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GEORGIA PERFORMANCE STANDARDS
SPS1. Students will investigate our current understanding of the atom.
b. Compare and contrast ionic and covalent bonds in terms of electron movement.
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THE BIG IDEA: TYPES OF CHEMICAL BONDS
ESSENTIAL QUESTION:WHY DO ATOMS FORM CHEMICAL
BONDS?
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TYPES OF CHEMICAL BONDS
Compound—substances made of the combined atoms of two or more elements.
Chemical formula—tells what elements a compound contains and the exact number of the atoms of those elements.
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TYPES OF CHEMICAL BONDS
Some Common Compounds
Vinegar Acetic acid HC2H3O2
Sand Silicon dioxide SiO2
Stomach Acid
Hydrochloric acid
HCl
Cane Sugar Sucrose C12H22O8
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TYPES OF CHEMICAL BONDS
Coefficient-Represents the #of units of each substance
2H2O
Subscript—represents # of atoms in a molecule of a particular element
SO42-
Superscript—represents oxidation # or how many electrons have been gained or lost.
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TYPES OF CHEMICAL BONDS
Atoms form compounds to become chemically stable. An atom is chemically stable when the outer energy level or valence shell is complete or full.
Chemical bond—force that holds together the atoms in a substance.
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TYPES OF CHEMICAL BONDS
Ionic Bond vs. Covalent Bonds
*loses or gains electrons
* Shares electrons
*attraction between opposite charges of ions
*can form multiple bonds
*between metal & nonmetals
Between a nonmetal and a nonmetal
** ION—positive or negatively charged atoms
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DO NOW:Chapter 20 Vocabulary:
1. Chemical bond2. Chemical
formula3. Ionic bond4. Covalent bond5. Molecule
See Pg. 626
6. Polar molecule7. Nonpolar molecule8. Oxidation number9. Polyatomic ion10. Ion
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GEORGIA PERFORMANCE STANDARDS
SPS1. Students will investigate our current understanding of the atom.
b. Compare and contrast ionic and covalent bonds in terms of electron movement.
![Page 14: UNIT 2 CHAPTER 20 CHEMICAL BONDS OCTOBER 5-9, 12-16, 2015.](https://reader038.fdocuments.in/reader038/viewer/2022103006/56649f1c5503460f94c331e5/html5/thumbnails/14.jpg)
THE BIG IDEA: ATOMIC BONDING
ESSENTIAL QUESTION:WHAT IS AN ION?
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ATOMIC BONDS
An atom that has lost or gained electrons is called an ion.
Ions are charged particles because it now has either more or fewer electrons than protons.
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ATOMIC BONDS
Ionic bonding occurs when an electron is donated.
loss of electron + called a cation
gain of electron - called an anion
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ATOMIC BONDSCovalent Bonding occurs when electrons are shared.
1. Single covalent bonds—2 shared electrons
2. Multiple covalent bonds—more than 1 pair of electrons.
3. Unequal sharing
polar bonds=unequal sharing, slightly +
nonpolar bonds=equal sharing
Watch video: Chemistry Basics Part 2
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DO NOW:
•COMPLETE THE QUIZ (OPEN NOTE)
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GEORGIA PERFORMANCE STANDARDS
SPS1. Students will investigate our current understanding of the atom.
b. Compare and contrast ionic and covalent bonds in terms of electron movement.
![Page 21: UNIT 2 CHAPTER 20 CHEMICAL BONDS OCTOBER 5-9, 12-16, 2015.](https://reader038.fdocuments.in/reader038/viewer/2022103006/56649f1c5503460f94c331e5/html5/thumbnails/21.jpg)
THE BIG IDEA: WRITING FORMULAS AND NAMING
COMPOUNDS
ESSENTIAL QUESTION:WHAT WOULD A CHEMIST NAME THE
COMPOUND CaCl?
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WRITING FORMULAS AND NAMING COMPOUNDS
Binary compound—compound composed of 2 elements
Oxidation number—positive or negative number (on PT) which indicates how many electrons an element has gained, lost or shared when bonding with another atom.
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WRITING FORMULAS AND NAMING COMPOUNDS
When writing formulas for binary ionic compounds, it is important to remember that compounds formed have a net charge of zero.
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WRITING FORMULAS AND NAMING COMPOUNDS
When writing formulas for binary ionic compounds, it is important to remember that compounds formed have a net charge of zero.
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WRITING FORMULAS AND NAMING COMPOUNDS
Polyatomic ions—a positively or negatively charged covalently bonded group of atoms.
The prefix poly—means “many” so the term polyatomic means “having many atoms.”
POLYATOMIC IONSCHARG
ENAME FORMULA
1+ AMMONIUM NH4+
1- ACETATE C2H3O2-
1- CHLORATE ClO3-
1-HYDROXID
EOH-
1- NITRATE NO3-
2-CARBONAT
ECO3
2-
2- SULFATE SO42-
3-PHOSPHAT
EPO4
3-
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WRITING FORMULAS AND NAMING COMPOUNDS
Hydrate—a compound that has water chemically attached to its ions and written into its chemical formula.
Covalent compounds can form more than one compound with each other. Scientists use Greek prefixes to indicate # of atoms of each element in binary compounds.
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WRITING FORMULAS AND NAMING COMPOUNDS
PREFIXES FOR BINARY COVALENT COMPOUNDS
# ATOMS
1 2 3 4 5 6 7 8
PREFIXMONO
-DI-
TRI-
TETRA-
PENTA-
HEXA-
HEPTA-
OCTA
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WRITING FORMULAS
•STEP 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number.
•STEP 2: Write the symbol of the element of the polyatomic ion with the negative oxidation number
•STEP 3: Add subscripts so that the sum of oxidation numbers of all atoms in the formula is zero—use the criss-cross method: the charge (without the sign) of one ion becomes the subscript of the other ion.
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NAMING COMPOUNDS•STEP 1: Write the name of the first element. (Subscripts do not become part of the name for the ionic compound but are used to determine prefixes when naming covalent compounds.)
•STEP 2: Write the root of the name of the second element. EX: Chlorine root is chlor-; oxygen root is ox-; bromine root is brom-
•STEP 3: Add the ending –ide to the root. Ex:
(Ionic) BaF2—Barium Fluoride, AlCl3—Aluminum
Chloride; (Covalent) N2O—Dinitrogen Monoxide,
CO—Carbon Monoxide
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DO NOW:
1. WHICH OF THESE ELEMENTS CONTAINS FOUR VALENCE ELECTRONS? A. HELIUM B. BERYLLIUM C. CARBON D. OXYGEN
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GEORGIA PERFORMANCE STANDARDS
SPS1. Students will investigate our current understanding of the atom.
b. Compare and contrast ionic and covalent bonds in terms of electron movement.
![Page 33: UNIT 2 CHAPTER 20 CHEMICAL BONDS OCTOBER 5-9, 12-16, 2015.](https://reader038.fdocuments.in/reader038/viewer/2022103006/56649f1c5503460f94c331e5/html5/thumbnails/33.jpg)
THE BIG IDEA: BONDING RULES/CHEMICAL
STRUCTURE
ESSENTIAL QUESTION:WHAT DOES “ENDS AND BENDS”
MEAN?
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BONDING RULES/CHEMICAL STRUCTURE
Hydrogen H—
Carbon —C
—
Nitrogen —N—
Oxygen —O
—
How many carbons?
Code# of
carbons
Examples
Meth- 1Methane (CH4)
Eth- 2 Ethane (C2H6)
Prop- 3Propane (C3H8)
But- 4Butane (C4H12)
Pent- 5Pentane (C5H12)
Hex- 6Hexane (C6H14)
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BONDING RULES/CHEMICAL STRUCTURE
Types of Carbon-Carbon BondsCode Means-ane Only carbon-carbon single bonds
-eneContain a carbon-carbon double
bondRule 1: Carbon lives on ends and bendsRule 2: Hydrogens bring carbon happinessWatch video: Making Sense of Chemical Structures
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GEORGIA PERFORMANCE STANDARDS
SPS1. Students will investigate our current understanding of the atom.
b. Compare and contrast ionic and covalent bonds in terms of electron movement.
![Page 38: UNIT 2 CHAPTER 20 CHEMICAL BONDS OCTOBER 5-9, 12-16, 2015.](https://reader038.fdocuments.in/reader038/viewer/2022103006/56649f1c5503460f94c331e5/html5/thumbnails/38.jpg)
THE BIG IDEA: REVIEW MAIN IDEAS OF CHAPTER 20
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CHAPTER 20 REVIEW
•ON A SEPARATE SHEET OF PAPER COMPLETE QUESTIONS #1-32