Section 1
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Mass Number
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Cards (142)
Section 1
(50 cards)
Mass Number
the sum of the number of neutrons and protons in an atomic nucleus
Mixtures
homogeneous or heterogeneous that can separate into components based on physical properties
Ion
a particle that is electrically charged (positive or negative) because it has gained or lost electrons. (protons not equal to electrons)
Carbonate
CO3 (2−)
Electron
negatively charged particle in the outer space of the atom that has a mass of 5.486x10^-4. (Its mass is so small that most ignore it)
Density
varies with temperature and is an identifying property
Elements
Atoms or molecules bound together (on periodic table)
Nitrite
NO2 (−)
Polyatomic Ions
tightly bound groups of atoms that behave as a unit and carry a charge
Cation
a positively charged ion
Permanganate
MnO4 (−)
Fahrenheit to Celsius
C = (F - 32)/1.8
Chlorate
ClO3 (−)
Hypochlorite
CIO (−)
Celsius to Fahrenheit
F = 1.8 (C) + 32
Atomic Number
The number of protons and electrons in a stable atom.
Iodate
IO3 (−)
Ionic Compound
composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal. (a metal and a non-metal)
Density Equation
Density = (mass)/(volume)
Thiocyanate
SCN (−)
Cyanide
CN (−)
Cathode Ray Experiment
This was JJ Thomson's experiment that led to the discovery of the electron and the development of the plum pudding model of the atom. The rays repelled by the negative electric field and the magnetic force causes the negative particle to move in circular motion.
Molecular Compound
a compound made up of two non metals; sharing electrons
Compounds
Pure substance that includes more than one element
Dichromate
Cr2O7 (2−)
Chlorite
ClO2 (−)
Heterogeneous Mixtures
mixture in which the composition is not uniform throughout
Hydrogen Sulfate (bisulfate)
HSO4 (−)
Naming Ionic Compounds
Metals are written 1st, non-metals last. Change the ending of non-metal to "ide" unless it is a polyatomic ion. Ignore the subscripts.
Homogeneous Mixtures
a mixture in which substances are evenly distributed throughout the mixture
Nitrate
NO3 (−)
Neutron
no charged particle in the nucleus that has a mass of about 1 amu
Acetate
CH3COO (−)
Hydride
H (−)
Naming Molecular Compounds
1. The name of the element to the left is named first 3. The name of the second element is given an -ide, unless polyatomic ion. 4. Greek prefixes should be used before both elements (Ex: dihydrogen triphosphide) 5. no "mono" for first element (Ex: carbon dioxide)
Perchlorate
CIO4 (−)
Celsius to Kelvin
K = C + 273.15
Bromate
BrO3 (−)
Oil Drop Experiment
Robert Millikan, suspended oil drops between charged plates, shot x-rays that put an electron on them, determined the smallest increment of charge difference needed to suspend the drops, and determined the charge on one electron
Isotope
an atom that has the same number of protons (or the same atomic number) as other atoms of the same element do but that has a different number of neutrons
Anion
a negatively charged ion
Gold Foil Experiment
Conducted by Ernest Rutherford in which alpha particles that were shot at gold foil were deflected when they hit the positive center of gold atoms. The nucleus was discovered as a result of this experiment.
Chromate
CrO4 (2−)
Dihydrogen Phosphate
H2PO4 (−)
Hydroxide
OH (−)
Molecule
two or more atoms held together by covalent bonds
Greek Prefixes for Molecular Compounds
mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
Proton
positively charged particle in the nucleus that has a mass of about 1 amu.
Hydrogen Carbonate (bicarbonate)
HCO3 (−)
Formate
HCOO (−)
Section 2
(50 cards)
Oxalate
C2O4 (2−)
Borate
BO3 (3−)
Oxidation Reaction
a chemical reaction in which a reactant loses one or more electrons such that the reactant becomes more positive in charge
Ammonium
NH4 (+)
Decomposition Reactions
complex substances are broken up into simpler substances (AB -> A+B)
Exergonic
chemical reaction that releases some form of energy, such as heat.
Net Ionic Equation
an equation that includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution (aka: removing ions that are on both sides of the equation)
Synthesis (Combination) Reactions
two or more substances combine to form a more complex substance (A+B -> AB)
Solubility Rules
1. Soluble Compounds - Anions if a compound contains one of the following Anions, they will be soluble: •Acetates •Chlorates •Perchlorates •Nitrates •Nitrites •Permanganates
Work
energy used to cause an object that has mass to move
Enthalpy
(thermodynamics) a thermodynamic quantity equal to the internal energy of a system plus the product of its volume and pressure
Pauli Exclusion Principle
no two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Neutralization Reaction
a chemical reaction in which an acid and a base interact with the formation of a salt and water (EX: HCl + NaOH --> NaCl (aka: the salt) + H2O (aka: water))
Naming Oxyacids
former suffix "ate;" root + ic. former suffix "ite;" root + ous. "i ATE ICky food at the whITE hOUSe." (EX: Perchlorate -> HCIO4: perchloric acid)
Heat
Energy used to cause the temperature of an object to rise
Precipitation Reaction
a reaction in which an insoluble substance forms and separates from the solution by combining two soluble substances.
Reduction Reaction
a reactant gains one or more electrons, thus becoming more negative in charge
Sulfite
SO3 (2−)
Solubility Rules (cont.)
2. Soluble Compounds - Cations if a compound contains one of the following Cations, it will be soluble. •NH4 (positive charge of 1) and Almost all of the Group 1A alkali Cations
Relationship of Energy to Work and Heat
Energy = heat + work
endothermic
describes a process in which heat is absorbed from the surroundings
Mercury I
Hg2 (2+)
Naming Binary Acids
1) Take root of second element, 1A) add "-hydro" prefix to the anion 1B) add "-ic" suffix" 2) Add acid as second word (EX: hydrochloric acid)
Potential Energy
energy stored due to an object's position or arrangement
Thiosulfate
S2O3 (2−)
Atomic Radius Trend
Across a period: decreases. Down a group: increases
Gas Forming Reactions
occur through the formation of a gas and water because both products remove ions from the solution; include carbonate, sulfite, Sulfide (all are polyatomic) and NH4OH (but last one is not as common).
Endergonic
A chemical reaction that requires the input of energy in order to proceed.
Sulfide
S (2−)
Arsenate
AsO4 (3−)
System
molecules chemist want to study
Solubility Rules (cont..)
3. Soluble Compounds with EXCEPTIONS If a compound contains one of the following Anions, they will be soluble: ------Chlorides, Bromides, Iodides {Except those compounds of Ag (+1), Hg2 (+2), and Pb (+2)} ------Sulfates {Except those compounds of Sr (2+), Ba (2+), Hg2 (2+), and Pb (2+)
Complete Ionic Equation
a reaction equation that shows all soluble compounds in their ionic forms (aka: it shows NaCl as Na+ and Cl−)
Combustion Reaction
a substance (most often a hydrocarbon) combines with oxygen, producing carbon dioxide and water
Solubility Rules (cont...)
4. Insoluble Compounds with EXCEPTIONS If a compound contains one of the following Anions, they will be insoluble: ------Carbonates, Phosphates, Sulfites {Except those compounds of NH4 (+), and alkali metals cations} ------Hydroxides, Sulfides {Except those compounds of NH4 (1+), alkali metals, and Ca (2+), Sr (2+), and Ba (2+)}
Surroundings
everything other than the system
Molecular Equations
A reaction equation which shows all soluble compunds in their ionic forms, a chemical equation written using the complete formulas of reactants and products (aka the original equation)
Exothermic
describes a process in which heat is released to the surroundings
Sulfate
SO4 (2−)
Hund's Rule
orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin
Kinetic Energy
the energy an object has due to its motion
Energy
the ability to do Work or transfer heat
Phosphate
PO4 (3−)
Peroxide
O2 (2−)
Phosphide
P (3−)
hydrogen phosphate
HPO4 (2−)
Nitride
N (3−)
Oxide
O (2−)
Exceptions to Hund's Rule
Chromium ([Ar] 4s1 3d5) Copper ([Ar] 4s1 3d10) molybdenum ([Kr] 5s1 4d5) Silver ([Kr] 5s1 4d10) Gold ([Xe] 6s1 4f14 5d10)
Arsenite
AsO3 (3−)
Section 3
(42 cards)