Exam Review Flashcards
Define metal
Shiny, good conductor, left of staircase, mostly solid, 1,2,3 valence electrons, lose electrons, mall, duct, grey, yellow, orange
Nonmetal
Dull, insulator, right of staircase, gain electrons, brittle, various colours
Metalloid
Semiconductors, share qualities of both, on staircase
Precipitate
Solid formed from the reaction of two solutions
Alkali metals
Group 1. Highly reactive, soft, shiny
Alkaline earth metals
Group 2 Light, reactive
Halogens
Group 17 Highly reactive
Noble gases
Group 18 Nonreactive
Chemical property
A description of what a substance does in a chemical reaction.
Physical property
Description of a substance without changing it into a new substance. Density, boiling point, melting point characteristic.
Bohr Diagram
Used to represent atomic structure. Nucleus contains # of protons and neutrons. Orbits drawn surrounding. Electrons drawn on. First, 2 at 12 o’clock. Second, max 8, filled clockwise at 3 o’clock, 6, 9. Go around twice. Same for next orbit, though it holds max of 18.
Lewis diagram
Element symbol in middle (including valence). Dots surround representing electron configuration in outer orbit.
Valence
Valence= ionic charge. Numeric value of electric charge on atom, followed by a plus or minus sign. Superscripted. Some metals have multiple valences.
Combining capacity
Number of other atoms a single atom can combine with chemically. Based on valence electrons, number in outer orbit. All atoms want to become stable. They achieve this by having a full outer orbit, or a stable octet. They do this by gaining, losing, or sharing electrons.
Ion
A charged atom. Formed when atoms gain or lose electrons.
Anion
Gains one or more electron, negatively charged (nonmetals) End of name changes to “ide”
Cation
Loses one or more electrons, positively charged (metals)
Electrolyte
A solution that conducts electricity. When ionic substances dissolve, their positive and negative ions are pulled away from each other by water molecules. Water surrounds the ions and prevents them from forming into compounds again.
Ionic bond
The attraction that holds oppositely charged The simultaneous strong attraction of positive and negative ions in an ionic compound. Very strong.
covalent bond
A bond that results from the sharing of outer electrons between nonmetal atoms. Both nuclei form strong attractions for each others electrons but are not strong enough to pull them away.
Ionic compound
Overall charge zero, electrically neutral.The total negative charges equals the total positive charges. Made up of cations and anions. Metals, with a weak hold on their valence electrons, transfer their valence electrons to non metals, with a strong hold on their valence electrons. Both have a stable electron configuration. Most are hard, brittle, solids with high melting points. Most are electrolytes. Do not exist as individual particles. Most form 3D crystals, with each ion held in fixed ratios.
Molecular compound
Nonmetals combine with nonmetals, held together by covalent bonds. Made up of individual molecules. Second element’s name ends with ide. Both get a prefix according to their number in the compound. The first element never gets the prefix “mono”
Chemical equation
A way of describing a chemical reaction using chemical formulas of the reactants and products. Provides more detail
Word equation
A way of describing a chemical reaction using the names or the reactants and products. Written out in full.
Skeletal equation
Not balanced. Shows reactants and products but the atoms are not in equal proportions.
Balanced equation
Obeys law of conservation of mass. Uses coefficients to account for all atoms. There are equal numbers of each atom on both sides of the equation.
Synthesis reaction
A reaction in which two reactants combine to make a larger or more complex product. A+B—->AB
Decomposition reaction
A reaction in which a larger or more complex substance breaks down to form two or more similar products. AB—–>A+B
Single displacement
An element displaces another element in a compound, producing a new compound and a new element. Often occur in aqueous solutions. Metals displace metals and non metals displace nonmetals. Metals displace H in acids.
Double displacement
A reaction that occurs when elements in different ionic compounds displace each other or exchange places, producing two new compounds. Many occur with two ionic compounds in solution. Many form a precipitate.
Coefficient
Placed before elements/compounds, give the ratio of reactants to products in a reaction.
Combustion
The rapid reaction of a substance with oxygen to produce oxides and energy. Aka burning.
Incomplete combustion
A combustion reaction of hydrocarbons that may produce carbon monoxide, carbon, carbon dioxide, water, and energy. Occurs when oxygen supply is limited. Orange, flickering flame as evidence.
Catalyst
Speeds up a chemical reaction but is not involved, goes above the arrow.
Acid
An aqueous solution that conducts electricity, tastes sour, turns blue litmus paper red, and neutralizes bases. Molecular compounds containing hydrogen and another nonmetal that form ions in water. Hydrogen ions give acids their properties, so acids only exist in aqueous solutions. Oxyacids are polyatomic ions combined with hydrogen, in solution.
Base
An aqueous solution that conducts electricity, is bitter, slippery, and turns red litmus paper blue.Many bases are ionic compounds dissolved in water containing hydroxide or carbonate ions. The anion gives bases their properties.
Indicator
A substance that changes its colour depending on the acidity or basicity of the solution.
pH
A measure of how acidic or basic a solution is. A scale from 0 to 14. 7 is neutral, 0 is highly acidic, 14 is highly basic. Acidity/ basicity is determined by concentration of hydrogen/hydroxide ions. A neutral solution has equal concentrations.
Neutralization reaction
A chemical reaction in which an acid and a base react to form an ionic compound (a salt) and water. The resulting pH is closer to 7. Usually a double displacement reaction.
Polyatomic compound
Contain at least one polyatomic ion (ions made up of more than one element) Anion named according to the ion, not individual elements.
Non electrolyte
A substance that does not conduct electricity when dissolved in water. Molecular compounds are non electrolytes.
Hydrocarbon
Compounds containing nothing but hydrogen and carbon. Usually originate from fossil fuels. Propane: C3H8 Methane: CH4 Octane: C8H18 Butane: C4H10
Polymer
Long chained molecules that have repeating units in them.
Metal oxide
A compound consisting of a metal and oxygen. Often a synthesis/synthesis reaction that releases energy.
Nonmetal oxide
A molecular compound where a nonmetal has reacted with oxygen.
Law of conservation of mass
In any given chemical reaction, the total mass of the reactants equals the total mass of the products.
Inhalation
Physically drawing air into the lungs
Exhalation
Physically pushing air out of the lungs
Lungs
Two sack like structures left and right of the heart containing air.
Trachea
Tube made of rings of cartilage below larynx, in front of esophagus, above left and right main stem bronchi. General passage for air from nasal cavity to bronchi.
Prokaryote
A single celled organism that does not contain a nucleus or other membrane bound organelles
Bronchus
Tube made of rings of cartilage branching left and right from trachea. Travels into left and right lung, branches into bronchioles.
Bronchiole
Branches from main stem bronchus throughout lungs, ends in alveoli.
Alveoli
End of terminal bronchiole. Balloon like, tiny sac of air in the lungs that is surrounded by a network of capillaries, where gas exchange takes place between air and blood.Thin walled
Cytokinesis
Cellular part of cell division. The cytoplasm and organelles divide to form two genetically identical cells.
Eukaryote
A cell that contains a nucleus and other membrane bound organelles. Can be thousands of times larger and be multicellular.
Diffusion
A transport mechanism for moving chemicals into and out of the cell, from an area of higher concentration to an area of lower concentration.
Surface area
Total area of all surfaces.
lxw)+(lxw