Exam 2 Material Test Questions – Flashcards
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| Chemical Bonds |
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| the attractive force that holds two atoms together in a more complex unit. |
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| Ionic Bond |
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| a chemical bond formed through the transfer of one or more electrons from one atom or group of atoms to another atom or group of atoms |
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| Ionic Compound |
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| a compound in which ionic bonds are present |
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| Covalent bond |
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| is a chemical bond formed through the sharing of one or more pairs of electrons between two atoms |
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| Covalent compound |
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| A molecular compound is a compound in which covalent bonds are present. |
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| Valence Electrons |
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| is an electron in the outermost electron shell of a representative element or noble-gas element. Participates in bonding. |
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| Lewis electron dot symbol |
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| The chemical symbol of an element surrounded by dots equal in number to the number of valence electrons present in atoms of the element. |
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| Group number |
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| an identifier used to describe the column of the standard periodic table in which the element appears. Example: Group 1: alkali metals Group 2: alkaline earth metals Group 17: halogens Group 18: noble gases |
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| Outermost electron shell |
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| The valence electron shell where bonding takes place |
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| Cation |
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| Positive Ion |
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| Anion |
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| Negative Ion |
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| Octet Rule |
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| In forming compounds, atoms of elements lose, gain, or share electrons in such a way as to produce a noble-gas electron configuration for each of the atoms involved |
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| isoelectronic series |
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| a group of atoms/ions that have the same number of electrons. Examples. N3-, O2-, F- |
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| ionic charge |
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| the electrical charge of an ion |
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| binary ionic |
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| is an ionic compound in which one element present is a metal and the other element present is a nonmetal. The metal is always present as the positive ion, and the nonmetal is always present as the negative ion. |
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| ternary ionic compounds |
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| consists of three compounds usually an element (i.e. metal) and a polyatomic ion. e.g. of ploy atomic ion Nitrate (NO3), Chlorate(ClO3), Chloric (ClO4), Sulphate (SO4) |
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| Chemical formula MxNy |
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| ? |
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| Polyatomic Ions |
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| A polyatomic ion is a molecule made up of 2 or more atoms that bears ionic groups, that is, a molecule with a charge. |
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| How many bonds can O form? |
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| 2 bonds |
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| How many bonds can H form? |
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| 1 bond |
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| Dipoles |
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| intermolecular force that occurs between polar molecules. |
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| lone pair of electrons |
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| a lone pair is a valence electron pair which is not shared with another atom and is sometimes called a non-bonding pair. |
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| VSEPR Theory |
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| a lone pair is a valence electron pair which is not shared with another atom and is sometimes called a non-bonding pair. |
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| Ab4 |
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| tetrahydral |
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| AB3E |
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| Pyramidal |
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| Ab2 |
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| linear |
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| AB2E2 |
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| angular or bent |
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| AB3 |
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| trigonal planar |
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| Single Bonds Double Bonds Triple Bonds |
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| bond with one pair of electrons bond with 2 bond with 3 |
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| sigma ? and pi ? bonds |
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| .A sigma bond is just a single bond. 2.When you have a double bond, you have 1 sigma bond and 1 pi bond. A pi bond is any bond formed after the single bond is formed |
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| mono di tri tetra penta hexa hepta octa nona deca |
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| 1 2 3 4 5 6 7 8 9 10 |
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| CO |
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| Carbon monoxide |
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| CO2 |
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| Carbon dioxide |
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| hybridization |
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| the idea that atomic orbitals fuse to form newly hybridized orbitals, which in turn, influences molecular geometry and bonding properties. |
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| Sp3 |
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| Tetrahydral 109.5 |
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| Sp2 |
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| trigonal planar 120 |
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| sp |
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| linear 180 |
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| molecular geometry |
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| shape of a molecule |
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| Electronegativity x |
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| hat describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself |
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| Boyle’s law |
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| PV = cnst |
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| ideal gas law |
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| Pv = nRT |
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| R |
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| Ideal gas constant |
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| amu |
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| 1.6606 x 10 ^ -24 |
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| charles law |
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| V/T=cnst |
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| Dalton's law |
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| Pt=Pa+Pb+Pc |
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| pressure |
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| force/area |
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| 1 atm |
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| 760 mm HG = 760 torr |
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| R |
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| 0.08205 (L atm)/(k mol) |
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| Avogrado's hypothesis |
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| V/n=cnst |
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| endothermic |
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| a process or reaction in which the system absorbs energy from its surroundings in the form of heat |
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| endergonic |
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| the total amount of energy is a loss (it takes more energy to start the reaction than what you get out of it) |
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| thermal expansion |
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| change in dimensions of a material resulting from a change in temperature. |
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| exogonic |
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| an action or object coming from within a system |
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| kinetic molecular theory |
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| experimental observations about gas |
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| exothermic |
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| a chemical or physical reaction that releases heat |
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| vapor pressure |
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| pressure of a vapor in thermodynamic equilibrium with its condensed phases in a closed container. |
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| compressibility |
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| a measure of the relative volume change of a fluid or solid as a response to a pressure (or mean stress) change. |
