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106 Terms

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Atom

The basic unit of a chemical element, consisting of a nucleus surrounded by electrons.

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Atomic Mass

The mass of an atom, typically expressed in atomic mass units (amu).

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Atomic Number

The number of protons in the nucleus of an atom, which determines the element's identity.

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Atomic Radius

The distance from the nucleus to the outermost electron shell of an atom.

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Avogadro’s Number

The number of atoms, molecules, or particles in one mole, approximately 6.022 × 10^23.

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Bonding Pair

A pair of electrons shared between two atoms in a covalent bond.

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Closed Shell

An electron shell that is completely filled with electrons.

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Compound

A substance made of two or more elements chemically bonded together.

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Electron

A subatomic particle with a negative charge, found in the electron cloud.

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Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

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Element

A pure substance consisting of only one type of atom.

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Energy Shells

The orbits or levels where electrons are found around the nucleus.

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Group

A vertical column in the periodic table.

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Ionic Bond

A chemical bond formed between two ions with opposite charges.

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Ionization Energy

The energy required to remove an electron from an atom or ion.

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Isotope

Atoms of the same element with different numbers of neutrons.

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Lewis Dot Structure

A diagram showing the bonding between atoms of a molecule and lone pairs of electrons.

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Lone Pair

A pair of valence electrons not shared with another atom.

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Mass Number

The total number of protons and neutrons in an atom's nucleus.

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Mechanical Mixture

A physical combination of substances that remain the same individual substances.

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Mixture

A combination of two or more substances that are not chemically bonded.

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Mole

A unit that measures the amount of a substance, based on the number of atoms or molecules.

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Molecule

A group of atoms bonded together, representing the smallest unit of a chemical compound.

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Neutron

A subatomic particle with no charge, found in the nucleus.

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Nonpolar Covalent Bond

A type of chemical bond where two atoms share a pair of electrons equally.

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Octet Rule

The principle that atoms tend to bond in such a way that they have eight electrons in their valence shell.

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Open Shell

An electron shell that is not completely filled with electrons.

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Period

A horizontal row in the periodic table.

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Polar Covalent Bond

A type of chemical bond where a pair of electrons is unequally shared between two atoms.

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Polyatomic Ion

An ion composed of two or more atoms covalently bonded.

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Proton

A subatomic particle with a positive charge, found in the nucleus.

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Pure substance

A substance that consists of only one type of particle.

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Quantum Mechanics

A fundamental theory in physics that describes the physical properties of nature at the scale of atoms and subatomic particles.

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Shared Electrons

Electrons that are shared between atoms in a covalent bond.

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Single, Double, Triple bonds

Types of covalent bonds involving one, two, or three shared pairs of electrons between atoms.

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Solution

A homogeneous mixture of two or more substances.

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Valence Electrons

Electrons in the outermost shell of an atom that are involved in chemical bonding.

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VSEPR Theory

A theory that predicts the shape of molecules based on the repulsion between electron pairs.

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Accuracy

The closeness of a measured value to its true value.

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Avogadro’s Number

The number of atoms, molecules, or particles in one mole, approximately 6.022 × 10^23.

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Conversion factors

Ratios used to convert from one unit to another.

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Directly Proportional

A relationship where one variable increases as the other increases.

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Ideal Gas Law

An equation of state of an ideal gas: PV=nRT.

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Indirectly Proportional

A relationship where one variable increases as the other decreases.

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Molar Mass

The mass of one mole of a substance.

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Mole

A unit that measures the amount of a substance, based on the number of atoms or molecules.

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Precision

The closeness of two or more measurements to each other.

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SATP

Standard Ambient Temperature and Pressure 24.79L

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Scientific Constant

A fixed value that describes a physical property.

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Scientific Notation

A way of expressing numbers that are too large or too small to be conveniently written in decimal form.

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Significant Figures

Digits in a number that carry meaningful contributions to its measurement accuracy.

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STP

Standard Temperature and Pressure 22.7L

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Uncertainty

An estimate of how much a measured or calculated value deviates from the true value.

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Unit conversions

Ratios used to convert from one unit to another.

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Acid-Base Neutralization

A reaction between an acid and a base to produce a salt and water.

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Chemical Reaction

A process in which substances react to form new substances.

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Coefficients

Numbers used to balance chemical equations.

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Combustion Reaction

A reaction where a substance reacts with oxygen, releasing energy as heat and light.

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Decomposition Reaction

A reaction where a single compound breaks down into two or more simpler substances.

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Double Replacement Reaction

A reaction where parts of two compounds exchange places to form two new compounds.

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Endothermic Reaction

A reaction that absorbs energy from its surroundings.

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Enthalpy

The heat content of a system at constant pressure.

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Excess Reagent

A reactant that remains after a chemical reaction is complete.

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Exothermic Reaction

A reaction that releases energy to its surroundings.

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Limiting Reagent

The reactant that is entirely consumed when the reaction goes to completion.

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Percent Purity

The ratio of the mass of pure product obtained to the theoretical mass.

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Percent Yield

The ratio of the actual yield to the theoretical yield expressed as a percentage.

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Products

Substances formed as the result of a chemical reaction.

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Reactants

Substances that undergo a chemical reaction.

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Single Replacement Reaction

A reaction where an element reacts with a compound, displacing an element from it.

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Stoichiometry

The calculation of reactants and products in chemical reactions.

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Subscripts

Numbers written below the line that tell how many atoms of a given type are in a compound.

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Synthesis Reaction

A reaction where two or more simple substances combine to form a more complex substance.

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Ionic solid

A solid composed of ions bonded together in a lattice structure.

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Ionization

The process by which an atom or molecule acquires a negative or positive charge by gaining or losing electrons.

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“Like dissolves like”

A principle stating that polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes.

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Aqueous Solution

A solution in which the solvent is water.

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Boiling

The transition of a liquid to a gas.

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Boiling Point

The temperature at which a liquid changes to a gas.

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Concentration

The amount of solute dissolved in a given volume of solvent.

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Condensing

The transition of a gas to a liquid.

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Crystal lattice

A structure in which ions are arranged in a repeating pattern.

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Dilution

The process of reducing the concentration of a solute in solution, usually by mixing with more solvent.

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Dipole moment

A measure of the separation of positive and negative charges in a molecule.

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Dipole-Dipole forces

Forces of attraction between polar molecules.

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Dissociation and Ionization

The separation of ions in a solution by the action of a solvent.

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Entropy

A measure of the disorder or randomness in a system.

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Freezing

The transition of a liquid to a solid.

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Gas

A state of matter with no fixed shape and no fixed volume.

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Homogenous Mixture

A mixture that has uniform composition and properties throughout.

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Hydrogen Bonds

A type of weak chemical bond formed between an electronegative atom and a hydrogen atom bound to another electronegative atom.

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Intermolecular forces

Forces of attraction between molecules.

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Ionic Bond

A chemical bond formed between two ions with opposite charges.

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Lewis-Dot Structures

A diagram showing the bonding between atoms of a molecule and lone pairs of electrons.

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Liquid

A state of matter with a definite volume but no definite shape.

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London forces

Weak intermolecular forces resulting from instantaneous dipoles in molecules.

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Melting

The transition of a solid to a liquid.

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Melting Point

The temperature at which a solid changes to a liquid.

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Molarity

A measure of the concentration of solute in a solution in terms of amount of substance in a given volume.

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Molecular solid

A solid composed of molecules held together by intermolecular forces.