Chemistry Unit 8 Test Questions – Flashcards
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Covalent/molecular compound
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containing two or more nonmetals sharing electrons
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covalent bond
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bond formed when 2 electrons are shared by two nonmetals
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molecule
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a molecule is the smallest particle in a covalent compound sample
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Lewis structural formula
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arrangement of electrons around atoms to show bonding.
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Exothermic
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process of losing/ releasing energy
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Endothermic
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process of gaining/ absorbing energy
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VSEPR model
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valence electron pairs push each other away to minimize repulsions, resulting in fixed shapes for molecules
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Polar covalent bond
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bond formed due to unequal sharing of electrons due to electronegativity differences
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bond length
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distance between two bonding nuclei
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bond dissociation energy (bond strength)
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Energy required to break a bond
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Saturated Hydrocarbon
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carbon-hydrogen compound consisting of C-C single bonds
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Unsaturated Hydrocarbon
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carbon-hydrogen compound consisting of C-C single and double/triple bonds
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Structural Formula
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lewis structure showing bonds and lone pair of electrons
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Empirical Formula
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formula that represents atoms using least ratio of subscripts
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Molecular Formula
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formula that represents atoms using the correct ratio of subscripts
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sigma bond
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the first bond between two atoms, formed in the region between two atoms
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pi bond
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bond formed in addition to a sigma bond in a region above and below the sigma bond
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Resonance
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equivalent lewis structures due to alternating double and single bonds
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expanded octet
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a central atom surrounded by more than 8 electrons
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hybridization sp, sp2, sp3
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mixing of atomic orbitals to form equal energy hybrid orbitals
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Formal charge
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Valence electrons - (electron dots + bonds)
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NH3
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Ammonia
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CH4
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Methane
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Greek prefixes
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Mono, di, tri, tetra, penta, hexa
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Covalent naming
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-IDE, second element Greek prefix
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Binary Acids
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Needs "H", -IDE=hydro--ic acid
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Oxyacids
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"O" (hypo--ite=hypo--ous) (--ite=--ous) (-ate=--ic) (per--ate=per--ic)
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Ionic naming
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Name -- (roman # trans) -- name anion (mono= -ide)
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Octet rule
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atoms lose, gain or share valence electrons to achieve a stable configuration of EIGHT valence electrons. Strict-FONC. Violators-H,Be,B
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SMS method
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1. Given a formula, choose a central atom. 2. Arrange the other atoms symmetrically around the central atom. 3. Draw the electron dot structure for each atom. 4. Connect the single dots on the central atom to a single dot an outer atom to form single bonds. 5. Redraw the structure with a single line for each shared electron pair. 6. For IONS, add an electron per negative charge and take away an electron per positive charge
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Teddy method
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1. TE - add up valence es for all the atoms 2. Arrange atoms symmetrically 3. Dashes are the bonds connect using lines 4. Dot the outer atoms to complete octets 5. Place remaining electrons on the central atom as pairs 6. Draw double or triple bonds if needed 7. Yes ! check if all electrons are placed correctly
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Linear Shapes
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-results from two atoms bonded together. (eg N2 ) -results when three atoms bond together with no unshared electron pairs on the center atom. (eg CO2). -bond angle of 180
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Trigonal planar shape
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-results when three atoms bond to a central atom with no unshared electron pairs on the central atom. (eg: BCl3 , COCl2 ,CH2O). -bond angle of 120
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Tetrahedral shape
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-results when four atoms bond to a central atom with no unshared electron pairs (CCl4 , CH4). -bond angle is 109.5
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Trigonal pyramidal shape
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-results when three atoms bond to a central atom with one unshared electron pair (NH3). -bond angle is 107.3
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Angular or bent
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-results from two atoms bonded to a central atom and two unshared electron pairs (H2O). -bond angle 104.5
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Electronegativity
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the ability of an atom in a bond to attract electrons. -increases across period and decreases down a group
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Polar covalent bond
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A covalent bond in which atoms have slight positive and negative charg
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Hybrid orbitals
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sp, sp2 and sp3 are formed by combining s and p type orbitals
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Linear
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A2 , AX , AX2
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Angular/bent
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AX2E , AX2E2
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Trigonal planar
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AX3
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Trigonal pyramidal
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AX3E
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Tetrahedral
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AX4
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Trigonal bipyramidal
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AX5
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Seesaw
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AX4E
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T-shaped
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AX3E2
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Octahedral
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AX6
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Square pyramidal
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AX5E1
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Square planar
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AX4E2
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Organic compound
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-element CARBON is the basis -Bonding in carbon compounds is very stable because it always forms FOUR bonds.
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hydrocarbon
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an organic compound that contains the elements CARBON and HYDROGEN.
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alkane hydrocarbons
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CnH2n+2 Methane: CH4 Ethane: C2H6 Propane: C3H8 Butane: C4H10
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alkene hydrocarbons
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CnH2n Ethene: C2H4 Propene: C3H6 Butene: C4H8
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alkyne hydrocarbons
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CnH2n-2 Ethyne: C2H2 Propyne: C3H4 Butyne: C4H6
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petroleum
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a complex mixture of alkanes ex. Gasoline
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substituted halocarbons
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fluorethane: C2H5F chloropropane: C3H7Cl Fluorethene: C2H3F Chloropropene: c3h5cl
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alcohols
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(HYDROXYL) Methanol: CH3OH Ethanol: C2H5OH Propanol: C3H7OH Butanol: C4H9OH
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condensation reaction
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two smaller organic molecules combine to form a more complex molecule, accompanied by the loss of a small molecule such as water
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hydrogenation reaction
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involves the addition of hydrogen atoms to carbon atoms in a double or triple bond -used to convert liquid unsaturated fats into saturated fats that are solid at room temperature
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polymer
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a large molecule consisting of many repeating structural units Natural: proteins, DNA, RNA, carbs Synthetic: PVC, plastic, nylon, kevlar, teflon
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CO2
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carbon dioxide
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CO
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carbon monoxide
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N2O
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dinitrogen monoxide
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N2O5
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dinitrogen pentoxide
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SF6
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sulfur hexafluoride
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N2O4
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dinitrogen tetroxide
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ClF3
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chlorine trifluoride
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PCl5
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phosphorus pentachloride
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SiO2
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silicon dioxide
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SO3
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sulfur trioxide
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sulfur dioxide
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SO2
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dinitrogen trioxide
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N2O3
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nitrogen monoxide
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NO
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sulfur tetrafluoride
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SF4
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carbon disulfide
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CS2
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oxygen difluoride
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OF2
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HCl
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hydrochloric acid
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hydrofluoric acid
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HF
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H2S
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hydrosulfuric acid
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hydroiodic acid
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HI
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HNO3
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nitric acid
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HC2H3O2
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Acetic acid
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sulfuric acid
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H2SO4
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phosphoric acid
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H3PO4
