Chapter 2: Chemical Bonds
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1 Ch 2 pg. 1 Chapter 2: Chemical Bonds Compound: A substance composed of two or more elements united chemically in definite proportions. Molecule: A chemical combination of two or more atoms. Chemical bonds: A strong attractive force that exists between atoms in a molecule. Chemical reaction: Processes in which one or more substances are converted into other substances; also called chemical change. Example of a chemical reaction: 2 NO + O 2 2 NO 2 Figure on the left taken from Zumdahl, Chemistry and the picture on the right Figure taken from BLB Chemistry; The Central Science
2 Ch 2 pg. 2 Valence Electrons: those electrons in the atom s outermost shell and are responsible for determining the atom s chemistry. Picture taken from Zumdahl, Chemistry The number of valence electrons that an atom has is equal to the group number. Noble Gases: Members of group 8A in the periodic table. Stable Valence Electron Configurations: Element 1 st Energy level 2 nd Energy level 3 rd Energy level 4 th Energy level He 2 electrons Ne 2 electrons 8 electrons Ar 2 electrons 8 electrons 8 electrons Kr 2 electrons 8 electrons 18 electrons 8 electrons
3 Ch 2 pg. 3 Octet Rule: A rule stating that bonded atoms tend to possess or share a total of eight valence-shell electrons. Any atom surround by eight valence electrons is very stable; similar in stability to the noble gases. Classes of Chemical Compounds: Ionic Compounds: A compound composed of cations and anions, held together by electrostatic attractions. Ions: Electrically charged atom or groups of atoms; ions can be positively or negatively charged, depending on whether electrons are lost (positive) or gained (negative) by the atom. Cation: A positively charged ion. Anion: A negatively charged ion. Electrostatic forces: The glue that holds ionic compounds together, opposite charges attract.
4 Ch 2 pg. 4 Picture taken from ( Covalent compounds: Formed by the sharing of valence electrons through covalent bonds. Covalent bonds: A bond formed between two or more atoms by sharing electrons. Molecular structure for sucrose, a covalent compound.
5 Ch 2 pg. 5 Lewis Dot Symbols: The chemical symbol for an element with a dot for each valence electron; also called electron-dot symbol. Table taken from BLB; Chemistry the Central Science. Example: Write Lewis symbols for the following elements: N, P, As, Al, and I. Ionic Compounds: Figure taken from BLB s Chemistry; The Central Science; 9 th edition.
6 Figure taken from BLB s Chemistry; The Central Science Ch 2 pg. 6
7 Ch 2 pg. 7 Ionic Bond: The attraction between cations and anions that hold the compound together. Chemical Formula: A notation that uses chemical symbols with numerical subscripts to convey the relative proportions of atoms of the different elements in a substance. Example: Give the chemical formula for the ionic compound formed between: a) Magnesium and Sulfur b) Calcium and Chlorine c) Aluminum and Oxygen Crossover Method: Used to predict the formula for an ionic compound. Summary for ionic compounds: Comprised between a metal and a nonmetal. Held together by electrostatic attraction NO BONDS! Use the crossover method to help predict chemical formulas for ionic compounds. Covalent Compounds: Covalent compounds are formed through the sharing of electrons so that each atom is surrounded by 8 valence electrons. This is accomplished by forming covalent bonds. Single Bond: A covalent bond involving one electron pair. Double Bond: A covalent bond involving two electron pairs. Triple Bond: A covalent bond involving three electron pairs.
8 Ch 2 pg. 8 Lewis Dot Structures: A representation of covalent bonding in a molecule that is drawn using Lewis symbols. Shared electron pairs are shown as lines, and unshared electron pairs are shown as pairs of dots. Only the valence-shell electrons are shown. Guidelines for writing Lewis Dot Structures: Picture taken from PHH; General Chemistry. Example: Write the Lewis Dot Structures for the following compounds: CH 4, BF 3, SO 2, CO, CH 3 CH 2 OH, and SO Isomers: Compounds whose molecules have the same overall composition but different structures. Example: C 4 H 10 O, Butanol and Diethyl ether.
9 Ch 2 pg. 9 Physical Properties of Butanol and Diethyl ether: Property Butanol Diethyl ether Molecular Formula C 4 H 10 O C 4 H 10 O Molecular Weight g/mol g/mol Boiling Point ºC 34.6 ºC Density g/ml g/ml Equal Sharing vs. Unequal Sharing: Polar: Means a separation of charge in a molecule. Polar molecules contain a region of positive charge and a region of negative charge. Nonpolar Covalent Bond: A covalent bond in which the electrons are shared equally. Picture taken from PHH; General Chemistry; 8 th edition Polar Covalent Bond: A covalent bond in which the electrons are not shared equally. Electronegativity: A measure of the ability of an atom that is bonded to another atom to attract electrons to itself.
10 Ch 2 pg. 10 Picture taken from PHH; General Chemistry Dipole: A molecule with one end having a slight negative charge and the other end having a slight positive charge, a polar molecule. Dipole moment: A measure of the separation between the positive and negative charges in polar molecules. Picture taken from BLB; Chemistry, The Central Science
11 Ch 2 pg. 11 Structures: Structural formulas: A formula that shows not only the number and kinds of atoms in the molecule but also the arrangement of the atoms. Types of Models Used to Represent Structures: Picture taken from PHH; General Chemistry
12 Ch 2 pg. 12 Space-Filling Models: Depicts what the molecule would look like if the atoms were scaled up in size. Ball-and-Stick Model: Shows the atoms as spheres and the bonds as sticks, and they accurately represent the angles at which the atoms are attached to one another within the molecule. Line Art: Assumes that any point of connection between lines is a carbon atom that contains sufficient bonded hydrogen atoms to achieve the four bonds necessary for carbon. Picture taken from PHH; General Chemistry
13 Ch 2 pg. 13 Example: Give the condensed structural formula and the molecular weight of the molecule whose ball-and-stick model is shown. Refer to the color scheme on the previous overhead. Picture taken from PHH; General Chemistry One Last Example: Below is the line art structure for aspirin. Predict the chemical formula for aspirin. O O O
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