 |
Term
| what is a polar covalent bond |
|
Definition
| a bond between two non-metals with different electronegativity |
|
|
Term
| what is a nonpolar covalent bond |
|
Definition
| A bond in which electrons are shared between elements having a difference in electronegativity of less than 0.5 |
|
|
Term
| what is electronegativity |
|
Definition
| the tendency of an atom or radical to attract electrons in the formation of an ionic bond. |
|
|
Term
|
Definition
| are a model in chemistry used to predict the shape of individual molecules based upon the extent of electron-pair electrostatic repulsion |
|
|
Term
| how to determine molecular polarity |
|
Definition
Step 1: Draw the molecular strulkcture
Step 2: assign the polarity of each of the bonds
step 3: adding the bond dipoles to determine the net molecular dipole
step 4: decide if the bond dipoles cancle. if they do cancle, the molecule is nonpolar |
|
|
Term
|
Definition
|
|
Term
|
Definition
| is the amount of pure substance containing the same number of chemical units as there are atoms in exactly 12 grams of carbon-12. |
|
|
Term
|
Definition
|
|
Term
| how to calculate the molar mass of a molecule |
|
Definition
When you look up the atomic weight of oxygen, you find it is 16.00 g. Therefore, the molar mass of oxygen is:
2 x 16.00 g = 32.00 g |
|
|
Term
| convert the number of particles to moles and mass |
|
Definition
| Mass x MM X Moles X (1mole = 6.022x1023 X # of particles |
|
|
Term
| stoichiometry involving mass |
|
Definition
| Mass of A x MM of A x Moles of A x coefficients of bal equ. x Moles of B x MM of B x mass of B |
|
|
Term
| what is limiting reactant |
|
Definition
| limits the amount of product that can be formed. |
|
|
Term
| what is thoeretical yeild |
|
Definition
the amount obtained in the reaction
multiply the amount of moles of the limiting reagent by the ratio of the limiting reagent and the synthesized product and by the molecular weight of the product. |
|
|
Term
|
Definition
amount of product obtained in a reaction
Percentage Yield = mass of Actual Yield x 100%
mass of Theoretical Yield
|
|
|
Term
|
Definition
| amount of chemical that you actually make |
|
|
Term
|
Definition
| a homogeneous mixture of one or more solutes dissolved in a solvent. |
|
|
Term
|
Definition
| he minor component in a solution, dissolved in the solvent. |
|
|
Term
|
Definition
| The liquid in which a solute is dissolved to form a solution. |
|
|
Term
| what does "like dissolve like" mean |
|
Definition
| polar solutes dissolve in polar solvents. Nonpolar solutes dissolve in nonpolar solvents. |
|
|
Term
| how can pressure and temperature effect the solubility of gas in a liquid |
|
Definition
| as the temp increased the solubility of gas decreases and pressure increases the solubility of the gas |
|
|
Term
| what are miscible liquids |
|
Definition
| two or more liquids that can be mixed and will remain mixed under normal conditions |
|
|
Term
| what are immiscible liquids |
|
Definition
| when two liquids so not mix with each other |
|
|
Term
| what happens when ionic solid molecules get dissolved in water |
|
Definition
| the water molecules pull the ions apart |
|
|
Term
| what are some ways to speed up dissolving solid in liquid |
|
Definition
heat up the mixtrure
stire the mixture
add more solute than, filter out the excess
crushn the solute to give it a greater surface area |
|
|
Term
| what does unsaturated mean |
|
Definition
| contains carbon-carbon double bonds |
|
|
Term
|
Definition
containing max amount of solute
has no carbon-carbon bonds |
|
|
Term
|
Definition
| increase of concentration beyond saturation point |
|
|
Term
|
Definition
| Make (a liquid) thinner or weaker by adding water or another solvent to it. |
|
|
Term
|
Definition
| A substance made by removing water or other diluting agent; a concentrated form of something, esp. food. |
|
|
Term
| what is mass percent concentration |
|
Definition
|
|
Term
| what is voume percent concentration |
|
Definition
|
|
Term
| what is mass by volume percent concentraion |
|
Definition
|
|
Term
|
Definition
| concentration measured by the number of moles of solute per liter of solution |
|
|
Term
|
Definition
|
|
Term
stoichiometry involving solutions
|
|
Definition
| M orV of A x (mol=MV(L) x Moles of A x coefficients of bal eq. x Moles of B x mol=MV(L) x Mor V of B |
|
|
Term
| what are four evidences for a chemical reaction |
|
Definition
1. temperature change
2.precipitate is observed if possible
3. formation of bubble or gas
4. color change |
|
|
Term
| general format of a chemical reaction |
|
Definition
| reactant1 + reactant2 + … → product1 + product2 + … |
|
|
Term
|
Definition
| A substance that takes part in and undergoes change during a reaction. |
|
|
Term
|
Definition
| A substance produced during a natural, chemical, or manufacturing process |
|
|
Term
| what are the labels for physical states |
|
Definition
(g) gas
(l) liquid
(s) solid
(aq) dissolved in water |
|
|
Term
| what are seven elements that occur naturally as diatomic molecules |
|
Definition
| Iodine (I), Bromine (Br), Chlorine (Cl), Florine (F), Oxygen (O), Nitrogen (N), and Hydrogen (H) |
|
|
Term
| what are some driving forces of chemical reactions |
|
Definition
heat
enery
entropy
equilibrium shift |
|
|
Term
|
Definition
A + B ---> AB Metal + nonmental ---> ionic compound
|
|
|
Term
|
Definition
AB ---> A + B
Metal carbonate ---> metal oxide + carbon Dioxide
|
|
|
Term
|
Definition
A + BC ----> AC + B
Metal1 + aq solution1 ---> metal2 + aq solution2 |
|
|
Term
|
Definition
AB + CD ---> AD + CB
aq solution1 + aq solution2 --> aq solution3 + precipitate |
|
|
Term
|
Definition
| The process or result of oxidizing or being oxidized. |
|
|
Term
|
Definition
| , is any process in which electrons are added to an atom or ion (as by removing oxygen or adding hydrogen) |
|
|
Term
|
Definition
O2(g) is a reactant and heat is given off.
|
|
|
Term
| solubility rule for ionic compound in water |
|
Definition
NO3- - All nitrates are soluble.
Cl- - All chlorides are soluble except AgCl, Hg2Cl2, and PbCl2.
SO42- - Most sulfates are soluble. Exceptions include BaSO4, PbSO4, and SrSO4.
CO32- - All carbonates are insoluble except NH4+ and those of the Group 1 elements.
OH- - All hydroxides are insoluble except those of the Group 1 elements, Ba(OH)2, and Sr(OH)2. Ca(OH)2 is slightly soluble.
S2- - All sulfides are insoluble except those of the Group 1 and Group 2 elements and NH4+. |
|
|
Term
|
Definition
| The ionized or ionizable constituents of a living cell, blood, or other organic matter. |
|
|
Term
| what is a strong electrolyte |
|
Definition
| a solute that completely, or almost completely, ionizes or dissociates in a solution |
|
|
Term
| what is a weak electrolyte |
|
Definition
| an electrolyte that does not completely dissociate in solution. |
|
|
Term
|
Definition
is a substance that will not dissociate into charged ions when dissolved in water.
will not conduct electricity
|
|
|
Term
| what is a molecular equation |
|
Definition
| s the equation where each compound the sum of oxidation numbers is 0. |
|
|
Term
| what is a complete ionic equation |
|
Definition
| used to describe the chemical reaction while also clearly indicating which of the reactants and/or products exist primarily as ions |
|
|
Term
| what is a net ionic equation |
|
Definition
| a chemical equation for a reaction which lists only those species participating in the reaction |
|
|
Term
| what is intermolecular force |
|
Definition
| are forces of attraction or repulsion which act between neighboring particles (atoms, molecules or ions) |
|
|
Term
| what are van der waals forces |
|
Definition
| relatively weak electric forces that attract neutral molecules to one another in gases, in liquefied and solidified gases, and in almost all organic liquids and solids |
|
|
Term
| what are dipole-dipole forces |
|
Definition
| are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule |
|
|
Term
|
Definition
| the electromagnetic attractive interaction of a hydrogen atom and an electronegative atom, such as nitrogen, oxygen or fluorine, |
|
|
Term
| what is the london dispersion force |
|
Definition
| a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles |
|
|
Term
| what are the general properties of a liquid |
|
Definition
has definite volume
takes shape of its container
not compressable
not in fixed position
|
|
|
Term
|
Definition
| The temperature at which a liquid boils and turns to vapor. |
|
|
Term
|
Definition
| The pressure of a vapor in contact with its liquid or solid form. |
|
|
Term
|
Definition
| The tension of the surface film of a liquid caused by the attraction of the particles in the surface layer by the bulk of the liquid,... |
|
|
Term
|
Definition
| The state of being thick, sticky, and semifluid in consistency, due to internal friction. |
|
|
Term
|
Definition
easy to compress
expand to fill their containers
occupy more space than liquids
|
|
|
Term
|
Definition
|
|
Term
|
Definition
V = constant x T
V1T2 = V2T1 |
|
|
Term
|
Definition
P = constant x T
P1T2 = P2T1 |
|
|
Term
|
Definition
|
|
Term
| daltons partial pressure law |
|
Definition
| Ptotal = P1 + P2 + P3 + .... |
|
|
Term
| what is kinetic theory of gases |
|
Definition
| gases consist of small particles in random motion |
|
|
Term
|
Definition
|
|
Term
|
Definition
| A hypothetical gas whose molecules occupy negligible space and have no interactions, and that consequently obeys the gas laws exactly. |
|
|
Term
| stoichiometry involving gas |
|
Definition
| V of A (gas) x PV = nRT / stp 22.4 L/mol x moles of A x coeficients of bal eq. x mole of B x PV = nRT/ stp 22.4 L/mol x V of B |
|
|
Term
| general properties of acid |
|
Definition
taste sour
turns blue litmus red
destroys chemical property of bases
conducts an electric current
evolve hydrogen gas
|
|
|
Term
| general properties of a base |
|
Definition
bitter taste
does not change color of litmus paper
destroy chemical properties of acids
conduct an electri current
feel slippery
|
|
|
Term
|
Definition
a substance which releases hydrogen ions (H+) in solution.
Eg hydrochloric acid (HCl) dissociates to give H+ ions and Cl- ions and so is an acid |
|
|
Term
|
Definition
| is a substance that when added to water increases the number of OH- ions in the water |
|
|
Term
what is a bronsted lowry base
|
|
Definition
| is defined as anything that accepts H1+ ions. |
|
|
Term
| what is bronsted lowry acid |
|
Definition
| anything that releases H1+ ions |
|
|
Term
| what is conjugate acid-base pair |
|
Definition
| refers to acids and bases with common features |
|
|
Term
| what is ionization constant of water |
|
Definition
|
|
Term
|
Definition
| measures how acidic or basic a substance is and ranges from 0 to 14. |
|
|
Term
|
Definition
| is a measure of hydroxide ion (OH-) concentration. |
|
|
Term
|
Definition
| Acid + Base ----> salt + water |
|
|
Term
| what is titration of acid and base |
|
Definition
| the determination of the concentration of an acid or base by exactly neutralizing the acid or base with an acid or base of known concentration |
|
|
Term
|
Definition
|
|
Term
|
Definition
| is a molecule that tends to either bind or release hydrogen ions in order to maintain a particular pH |
|
|
Term
| what is an organic compound |
|
Definition
| low melting point, not soluble in H2O, slow reactions |
|
|
Term
|
Definition
| contains only carbon and hydrogen atoms |
|
|
Term
| prefixes associated with the number of carbon atoms in an organic compund |
|
Definition
| 1-meth, 2-eth, 3-prop, 4-but, 5-pent, 6-hex, 7-hept, 8-oct, 9-non, 10-dec |
|
|
Term
| what is a molecular formula |
|
Definition
| name of compounds or atoms |
|
|
Term
| what is a fully expanded formula |
|
Definition
|
|
Term
| what is a condensed formula |
|
Definition
|
|
Term
| what is a bond line formula |
|
Definition
The skeletal formula of an organic compound is a shorthand representation of its molecular structure
[image] |
|
|
Term
| structures and names of different funtional groups |
|
Definition
|
|
Term
| what are primary(1o), secondary (2o), Tertiary (3o) alcohols |
|
Definition
|
|
Term
| what are primary, secondary, tertirary amines |
|
Definition
|
|
Term
|
Definition
| a single bond, tetrahedral 109.5o bond angle |
|
|
Term
|
Definition
| ass suffix "ane" substiituents end with "yl" |
|
|
Term
| physical properties of alkanes |
|
Definition
molecular polarity: larger the alkane the more polar it is
boiling and melting points:
[image] |
|
|
Term
|
Definition
| contain one or more carbon double bonds |
|
|
Term
|
Definition
add "ene" at the end of name, arrange alpha order, souble bond to two diffenerent groups use cis-trans
Cis = same
trans = opposite |
|
|
Term
|
Definition
one or more triple bonds
180o |
|
|
Term
|
Definition
|
|
Term
|
Definition
| a saturated hydrocarbon that contains carbon atoms bonded to form a ring |
|
|
Term
| how to name a cycloalkane |
|
Definition
CnH2n single bonds
same sum letter that comes first in the alphabet goes first |
|
|
Term
| how to name a cycloalkene |
|
Definition
CnH2n
same sum letter that come first in alphabet goes first |
|
|
Term
| what is an aromatic hydrocarbon (benzene) |
|
Definition
| used to classify benzene and its derivatives |
|
|
Term
how to name an aromatic hydrocarbon
|
|
Definition
|
|
Term
| what is a chiral or achiral center |
|
Definition
| achiral does not have 4 different substituents |
|
|
Term
|
Definition
| chiral carbon that contains 4 different substituents |
|
|
Term
|
Definition
| a compound displaying isomerism with one or more other compounds |
|
|
Term
what are consitutional isomers
|
|
Definition
| molecules having the same molecular formula but different arangments of atoms |
|
|
Term
|
Definition
| isomers that have the same connectivity but different orientations of their atoms in space |
|
|
Term
| determine the maximum possible number of stereoisomers |
|
Definition
| calculate 2n, n = # of stereocenters |
|
|
Term
| how many stereoisomers are usually active in biological system |
|
Definition
|
|
Term
| what ate configurational isomers |
|
Definition
| a subcategory of stereoisomers that posses the same molecular formula, same connectivity but differ spatially due to internal bond rotation |
|
|
Term
|
Definition
| Each of a pair of molecules that are mirror images of each other. |
|
|
Term
| what is the one property that enantimers differ in |
|
Definition
| they're interacting with other chiral substances. |
|
|
Term
| what is a racemic mixture |
|
Definition
| is one that has equal amounts of left and right-handed enantiomers of a chiral molecule.... |
|
|
Term
|
Definition
| stereoisomers that are not mirror images of one another and are non-superimposable on one another. |
|
|
Term
| what are conformational isomers |
|
Definition
| is a form of stereoisomerism in which the isomers can be interconverted exclusively by rotations... |
|
|
Term
| what are axial or equatorial groups |
|
Definition
| is axial (straight up or straight down) and the other group is equatorial (at an angle, up or down). |
|
|
Term
| what is the 1,3-diaxial interaction |
|
Definition
| n interaction (usually repulsive) between two axial substituents on a cyclohexane ring. |
|
|
