Flashcards

Chem Exam Review Notes

Gagneet Grewal English 89 cards

Cards in this deck (89)

1Element Definitionis a pure substance that cannot be broken down into simpler substances by chemical
means and is composed entirely of only one kind of atom
2MetalsElements that conduct heat/electricity, are malleable, ductile, and lustrous
3Non-MetalsElements that are non-conductive and brittle as solids
4MetalloidsElements that have share metallic and nonmetallic properties
5Modern Periodic Lawstates that when elements
are arranged in order of their increasing atomic number, their properties show a periodic recurrence and gradual change.
6Groupis a vertical column in the periodic
table with elements that share similar
chemical properties.
7Periodis a horizontal row of elements
whose properties change from metallic on
the left to nonmetallic on the right.
8Protonis a positively charged subatomic particle in the nucleus of an atom.
9Electronis a negatively charged subatomic particle.
10Neutronis an uncharged subatomic particle in the
nucleus of an atom
11Atomic Numberis the number of protons present in the nucleus of an atom of a given element.
-The number of electrons equals the number of protons in an atom.
12Atomic Massis the sum of the number of protons and neutrons present in the nucleus of an atom.
number of neutrons = mass number – atomic number
13Isotopesare atoms of an element that differ from each other only in the number of neutrons in their nuclei.
14Isotopic Abundancerefers to the percentage of naturally-occurring isotopes of an element. The listed atomic mass of an element is the weighted average of its isotopes.
15Ground Stateis the lowest energy level that an electron can occupy.
16Transitionis a movement from one energy level to another.
17Valence Electronsare those electrons in the highest energy level of an atom.
18Atomic RadiusThe distance between the nuclei of bonded or adjacent atoms of the same element divided by two represents the
atomic radius of an element.
19Atomic Radius Down a Groupthe atomic radius gets larger (adds on
extra shell; inner electrons cause shielding of the nucleus)
20Atomic Radius Across a Periodthe atomic radius gets smaller (more
protons added to nucleus increases effective nuclear charge)
21Diagram for Atomic Radius
22Ionization Energythe amount of energy required to REMOVE an electron from an atom or ion in the gaseous state
23Ionization Energy Down a Groupsince the electrons are further from the nucleus, they are more loosely held and easier to remove
So the ionization energy decreases down a group.
24Ionization Energy Across a Periodsince the electrons are closer to the nucleus, they are more tightly held and harder to remove
So the ionization energy increases across a period
25Diagram for Ionization Energy
26Electron Affinitythe energy released when an electron is accepted by an atom in the gaseous state
27Electron Affinity Down a GroupAs atomic radius increases, the atom has looser hold on electrons, the electron affinity decreases.
-down a group, EA decreases
28Electron Affinity Across a PeriodAs atomic radius decreases, the atom has tighter hold on electrons, the electron affinity increases.
-across a period, EA increases
29Diagram for Electron Affinity
30Electronegativity in Periodic Trendan atom's ability to attract and bind with electrons.
31Diagram for Electronegativity
32Activity Series: Reactivityis a chemical property of an element that indicates the tendency of the element to form a compound.
-an element that forms compounds easily has high reactivity
-an element that does not form compounds has low reactivity
33Activity Seriesis a list of elements in order of their
reactivity, based on evidence gathered from single displacement reactions.
34Single Displacements Reactivityis a list of elements in order of their
reactivity, based on evidence gathered from single displacement reactions.
35Single Displacement Reactions in Activity Serieswill only occur if the reactant element has higher reactivity (higher in the activity series) than the element to be displaced
36Ionic Compoundsare pure substances
composed of ions and formed by the
transfer of electrons from a metal and a
nonmetal.
37Ionic Bondsare a type of chemical
bond created due to the electrostatic
attraction between positive and
negative ions.
38Octet Rulestates that representative
elements want a stable octet consisting of
a full shell of eight electrons in their outer
energy level.
39Molecular Compoundsare pure substances composed of two or
more nonmetals.
40Covalent Bondsare a type of chemical bond created by an
attractive force between two atoms when they share electrons.
41Classical Name and IUPAC Name Chart
42Polyatomic Ionis a group of atoms covalently bonded together that carry an overall charge due to the presence of extra electrons
(anion) or a deficiency in electrons (cation).
43Chemical Changeare any changes in which a new substance is formed.
44Chemical Equationrepresents a reaction by indicating the chemical formular, number of entities,
and states of matter of the reactants and products.
45Combustion and Synthesis ReactionTwo or more reactants unite to form a single product.
46Complete Combustionis when the substance is completely burned and only carbon dioxide and water remain.
47Incomplete Combustionis the type of combustion that leads to the production of carbon monoxide.
hydrocarbon + oxygen gas -> carbon dioxide + water + carbon monoxide + carbon (soot)
48Electronegativity: Polar Covalent Bondsis a property of an atom within a covalent bond describing its ability to attract
the electrons in the bond to its nucleus
49NonPolar Covalent Bondresults from a zero difference in electronegativity between the bonded atoms and has equal sharing of bonding electrons.
50Polar Covalent Bondresults from a difference in electronegativity between the bonded atoms and the electrons are not shared equally.
-results in partial positive and negative ends of the bond called dipoles (S+ and S-)
51Ionic BondWhen the electronegativity difference is high, the bonding pair of electrons is mostly with one atom/ion resulting in an ionic bond
EN= 1.7>
52NonPolar Moleculehas either all nonpolar bonds or polar bonds whose bond dipoles cancel, such that there is no positive/negative ends. Dipole is 0.
H-H -> H2
53Polar Moleculehas polar bonds with
dipoles that do not cancel and create
positive and negative ends of the molecule.
54Intramolecular ForcesForce which keeps molecules together
55Intermolecular ForcesAttractive force between molecules. Responsible for keeping matter in solid or liquid phase.
56Types of Intermolecular ForcesThese forces of attraction (and repulsion) between molecules are generally much weaker than covalent and ionic bonds (intramolecular forces).
57Dipole Dipole Forcesa force of attraction between polar molecules where the oppositely charged dipoles attract one another
-the greater the polarity of the molecule, the greater the strength of the dipole-dipole force
58Hydrogen Bondsis the attractive force between the hydrogen attached to an electronegative atom of one molecule and an electronegative atom of a different molecule.
59London-Dispersion ForcesA brief imbalance of electrons on one side of a molecule causing the neighboring molecule to be attracted. These are very weak, temporary forces.
60Size and shape of Intermolecular ForcesThe larger the size, the greater the intermolecular forces.
The more irregular the shape the weaker the intermolecular force.
ULTIMATELY, the greater the surface area, the stronger the intermolecular force
61Electrical Conductivitythe ability of a substance or an object to allow an electric current to exist within it.
62Ionic Compounds and Electrical ConductivityIonic compounds dissolved in water conduct electric current because the ions are free. This allows electrons to flow. The negative ions will orient themselves to the positive electrodes and positive ions will orient themselves to the negative electrodes
63Homogeneous Mixturescomposed of at least one solute (substance that gets dissolved) and one solvent (substance that does the dissolving).
64Importance of Being Water1. highly polar compound (large difference in electronegativity)
2. capacity for hydrogen bonds (two donor, s+, and two acceptor, S-)
3. Small Size of Molecules
65Solubilityis a quantitative property of a solute that measures how much of that substance can be dissolved in a solvent at a specific temperature and pressure.
-measured in g/100 mL
66Solutionis a homogenous mixture. The simplest solutions contain two substances. Most common solutions contain many substances.
67Solventis a substance that dissolves a solute (a chemically different liquid, solid or gas), resulting in a solution. A solvent is usually a liquid, but can also be a solid or a gas.
68Two Basic Components of a SolutionSolvent and Solute
69Concentrated Solutionis a solution that contains a large amount of solute relative to the amount that could dissolve (denser).
70Dilute Solutionhas a low concentration of the solute compared to the solvent (less dense).
71Saturated Solutioncannot dissolve more solute, all solute is dissolved!
72Unsaturated Solutiona solution that is capable of dissolving more solute, all solute is dissolved!
73Supersaturated Solutionis a solution that contains more solute than it should, which results in a highly unstable solution.
74Aqueous Solutionis a solution in which water is the solvent.
753 Factors that Affect Rate of Dissolving1. Temperature
2. Agitation
3. Particle Size
76TemperatureIn fact, for most solid solutes; the rate of dissolving is greater at higher temperatures. At higher temperatures, the solvent molecules have greater kinetic energy. Thus, they collide with the undissolved solid molecules more frequently.
77Agitationagitating a mixture by stirring or by shaking the container increases the rate of dissolving.
78Particle Sizedecreasing the size of the particles increases the rate of dissolving
79Polar CompoundA bond between 2 non-metal atoms that have the same electronegativity and therefore have equal sharing of the bonding electron pair
80NonPolar CompoundA bond between 2 non-metal atoms that have different electronegativities and therefore have unequal sharing of the bonding electron pair
81Solubility of Covalent CompoundsMany covalent compounds do not have negative and positive charges to attract water molecules. Thus, they are not soluble in water.
82Non-electrolytesdo not conduct electricity when dissolved in water.
83Volumetric Flaskis a pear-shaped glass container with a ﬂat bottom and a long neck.
84Ion Charge and SolubilityCompounds of ions with small charges tend to be soluble. Compounds of ions with large charges tend to be insoluble. Why? Increasing the charge increases the force that holds the ions together.
85Ion Size and SolubilitySmall ions bond more closely together than large ions. Thus, the bond between small ions is stronger than the bond between large ions with the same charge. As a result, compounds with small ions tend to be less soluble than compounds with large ions.
86Double Displacement Reactions that produce a precipitateA double displacement reaction that results in the formation of an insoluble substance is often called a precipitation reaction.
87Spectator Ionsis an ion that exists as a reactant and a product in a chemical equation.
88Arrhenius theory of Acids and BasesAn acid is a substance that dissociates in water to produce one or more hydrogen ions, H+. • A base is a substance that dissociates in water to form one or more hydroxide ions, OH−. Neutralization happens because H+ ions and OH- ions react to produce H2O.
89Bronsted-Lowry Theory of Acids and BasesAn acid is a substance from which a proton (H+ ion) can be removed. A base is a substance that can remove a proton (H+ ion) from an acid. An acid is a proton (hydrogen ion) donor. A base is a proton (hydrogen ion) acceptor.