finals review for the worst class on earth

Charles‘s Law

The volume of a gas increases with increasing temperature as long as the pressure does not change

Pressure

Increasing ____ raises the boiling point of a liquid.

Double covalent bond

covalent bond formed by atoms that share two pairs of electrons

Triple covalent bond

Covalent bond formed by atoms that share three pairs of electrons

Silicon

Which element is most likely to form covalent bonds?

• silicon (14)

• Oxygen (8)

• Chlorine (17)

• Sulfur (16)

Identical to

The energy released in the formation of a compound from its elements is always ___ the energy requirements decompose that compound into its elements

Boyle‘s law

The pressure of a gas will increase as the volume of the container decreases provided temperature does not change

Bernoullis principle

Fluid velocity increases when the flow of the fluid is restricted

Pascals principle

Pressure applied to a fluid is transmitted throughout the fluid

Archimedes‘ Principle

Buoyant force on an object is equal to the weight of the fluid displaced by the object

Suspension

Heterogeneous mixture containing a liquid in which you can see particles settle

Kinetic theory of matter

Matter is Made up of small particles that are in constant motion

Amorphous solid

• Liquid: soften and gradually turn to liquid over time

• Solid: Lacks a crystalline structure and doesn’t have a specific melting temperature

• Ex: glass, butter

Liquid crystal

• Liquid: flows like a liquid in the liquid phase, but doesn’t lose geometric arrangement

• Solid: Retains geometric arrangement in specific directions

• Ex: cellphones, calculators

Melting point

The temperature at which a solid begins to turn into a liquid

Heat of fusion

The amount of energy needed to change a substance from a solid to a liquid at its melting point

Boiling point

The temperature at which the pressure of the vapor in a liquid is equal to the external pressure acting on the surface of a liquid

Heat of vaporization

• The amount of energy needed for a liquid at its boiling point to become a gas

• Requires energy to be added to the substance

Sublimation

The change from a solid to a gas without a liquid state

Plasma

• Matter consisting of positively and negatively charged particles

• Most abundant matter in the universe

• Has enough energy to overcome attractive forces between its particles and within atoms

Thermal expansion

An increase in size of a substance when temperature is increased

Buoyancy

The ability of a fluid (a liquid or gas) to exert an upward force on an object immersed in it

Pressure

• force extorted per unit area

• Pressure (Pa) = Force (N) / area (m²)

• Input force (N) / input area (m²) = output force (N) / output area (m²)

Viscosity

The resistance of a fluid to flowing

Substance

A pure form of matter that has a uniform composition and specific properties

Compound

• A substance in which two or more elements are combined in a fixed proportion

• Electrically neutral

Dinitrogen oxide

What is the name of N2O?

Greek

____________________ prefixes are used to indicate how many atoms of each element are in a binary covalent compound.

Homogeneous mixture

• Contains two or more substances blended evenly throughout

• Can be separated by physical changes

Heterogeneous mixture

Mixture in which different materials can easily be distinguished

Solution

• Homogeneous mixture of particles too small to see with a microscope and too small to settle

• Won’t scatter light

Tyndall effect

Observed When light passes through a colloid

Colloid

• A mixture with particles visible under a microscope

• not heavy enough to settle

• Scatters light

• Example: smoke

• Not homogeneous

Physical property

• A characteristic that can be observed without changing the substance

• Examples: odor, color

Physical change

A change in size, shape, or state of matter, but not a change in the substance

Chemical change

A change of one substance to another

Chemical property

• A characteristic that indicates whether a substance can change to another substance

• Examples: flammability, color change, temperature change

Distillation

The separation of substances in a mixture using evaporation

Law of conservation of mass

The mass of a substance before a chemical change equals the mass of all substances after the change

Atom

The smallest particle of an element that retains the element‘s properties

Nucleus

The small, positively charged center of an atom

Proton

Particles in the nucleus with an electric charge of 1+

Neutron

Electrically neutral particles in the nucleus

Electron

Particles with an electric charge of 1-

Quark

Smaller particles that make up protons and neutrons

Electron cloud

• The area around the nucleus where electrons are most likely to be found

• NOT called the negative zone

Atomic number

The number of protons in the nucleus of an atom

Probability cloud

What best represent the location of an electron in an atom according to modern atomic theory

Mass number

The sum of protons and neutrons in an atom’s nucleus

Isotope

Atoms of the same element with different numbers of neutrons

Average atomic mass

The weighted average mass of all naturally occurring isotopes on an element (amu)

Periodic table

The chart that categorizes all known elements in rows and columns, based on their atomic number and recurring chemical properties

Period

The horizontal rows of elements in the periodic table that are numbered 1-7

Group

The vertical columns in the periodic table that are numbered 1-18

Halogens

• group 17 of periodic table

• Form diatomic molecules in gaseous state

Electron dot diagram

Uses the chemical symbol of an element surrounded by dots to represent the number of electrons in the outermost energy level

Selenium

Element in the oxygen group that is needed in trace amounts in your diet

Actinides

• Second row of inner transition elements

• atomic numbers 90 through 103

• named derived from the element actinium.

• radioactive, unstable, rare, and nonexistent in nature

• Where most synthetic elements are found

Lanthanides

• First row of the inner transition elements

• atomic numbers 58 through 71

• name is derived from the element lanthanum

Metal

• Elements that are shiny, malleable, ductile, and good conductors of heat and electricity, solid at room temperature (except for mercury)

• 1-2 electrons in outer electron shells

• Include alkali metals, alkaline earth metals, iron triad, boron group, carbon group, and nitrogen group

Malleable

The ability metals have that allows them to be rolled or hammered into sheets

Ductile

The ability metals have that allows them to be drawn into wire

Metallic bonding

• Positively charged metallic ions are surrounded by a sea of electrons

Radioactive element

An element in which the nucleus breaks down and gives off particles and energy

Transition element

• Elements groups 3-12 in the periodic table

• Often occur as uncombined elements in nature

Boron

Only element in group 13 that is NOT a metal

Nonmetal

• Element that is usually a gas or solid at room temperature

• Found on the far right of the periodic table

• Includes halogens and oxygen group

Diatomic molecule

• Consists of two atoms in a covalent bond

• Can be two of the same element (O2) or one atom of two different elements (CO)

Metalloid

• Elements that have both properties of metals and nonmetals

• Most likely to be semiconductors

Allotrope

Different molecular structures of the same element

Semiconductor

Elements that conduct electricity under certain conditions only

Transuranium element

Elements that have more than 92 protons

Chemical formula

Shows what elements a compound contains + the exact number of the atoms of each element in a unit of that compound

Chemical bond

The force that holds atoms together in a compound

Ion

A charged particle that has either more or fewer electrons than it has protons

Ionic bond

The force of attraction between a positive ion and a negative ion in an ionic compound

Covalent bond

The force of attraction between two atoms that share electrons

Molecule

• The neutral particle that forms when atoms share electrons

• Two or more atoms are bonded together

Nonpolar bond

A covalent bond where the electrons are shared equally

Polar bond

A covalent bond where electrons are unequally shared producing charged molecule ends

Polar molecule

A molecule that has a slightly positive end and a slightly negative end, but the molecule itself is neutral

Nonpolar molecule

A molecule in which the electrons are shared equally between atoms in the chemical bond

Oxidation number

A positive or negative number that indicates how many electrons an atom has gained, lost, or shared to become neutral

Binary compound

The easiest compounds to write formulas for, composed of two elements

Polyatomic ion

A positively or negatively charged group of covalently bonded groups of atoms

Hydrate

A compound that has water chemically attached to its atoms and written in its chemical formula

Chemical reaction

A change in which one or more substances are converted into new substances

Pure substance

Consists of only one kind of atom or only one kind of molecule

Reactants

The starting substances that react in a chemical reaction

Products

The new substances produced from a chemical reaction

Chemical equation

A way to describe a chemical reaction using chemical formulas and other symbols

Coefficient

Represent the number of units of each substance taking part in a reaction

Balanced chemical equation

A chemical equation with the same number of atoms of each element on both sides of the arrow

Mole

The amount of a substance that contains 6.02 × 10²³ particles of that substance

Molar mass

The mass (g) of one mole of a substance

Combustion reaction

A reaction in which a substance reacts with oxygen to produce heat and light

Synthesis reaction

A reaction in which two or more substances combine to form another substance

Decomposition reaction

A reaction in which one substance breaks down, or decomposes, into two or more substances

Single-displacement reaction

A reaction in which one element replaces another element in a compound

Double-displacement reaction

A reaction in which the positive ion of one compound replaces the positive ion of the other compound to form two new compounds