Science Review Flashcards

Atom

The basic building block of matter.

Proton

Positively charged subatomic particle located in the nucleus.

Neutron

Neutral subatomic particle located in the nucleus.

Electron

Negatively charged subatomic particle orbiting the nucleus.

Nucleus

The central part of an atom, containing protons and neutrons.

Atomic Mass Calculation

Add the number of protons and neutrons in the atom.

John Dalton's Atomic Theory Contribution

Atoms make up elements and are extremely small particles.

Niels Bohr's Atomic Theory Contribution

Electrons are found in different energy levels around the nucleus.

Ernest Rutherford's Atomic Theory Contribution

Most of the mass of an atom is in the center (nucleus), and the rest is empty space.

Erwin Schrodinger's Atomic Theory Contribution

Proposed the quantum model and the idea of the electron cloud.

Chemical Symbol

A one- or two-letter abbreviation for a chemical element.

Chemical Name

The scientific name for a chemical element or compound.

Atomic Number

The number of protons in the nucleus of an atom.

Atomic Mass

The total mass of protons and neutrons in an atom.

Group (Periodic Table)

A vertical column of elements in the periodic table with similar chemical properties.

Period (Periodic Table)

A horizontal row of elements in the periodic table.

Physical Property

A characteristic of a substance that can be observed or measured without changing the substance's chemical identity.

Chemical Property

A characteristic of a substance that determines how it reacts with other substances.

Liquid Halogen

Bromine

Halogens Group Number

Group 17

Noble Gases Group Number

Group 18

Iron's Group Number

Group 8

Element at Group 16, Period 3

Sulfur

Reactivity (Chemical Property)

The ability of a substance to react with other substances.

Flammability (Chemical Property)

The ability of a substance to burn in the presence of oxygen.

Toxicity (Chemical Property)

The ability of a substance to cause harm to living organisms.

Conductor

A material that allows heat or electricity to flow through it easily.

Semiconductor

A material that has electrical conductivity between that of a conductor and an insulator.

Ductility

The ability of a substance to be drawn into wires.

Malleability

The ability of a substance to be hammered into thin sheets.

Luster

The shininess of a substance.

Most Reactive Group of Metals

Alkali Metals

State of Alkaline Earth Metals in Nature

Only found as compounds in nature

Key Properties of Transition Metals

Shiny, malleable, ductile, dense, good conductor, React by losing electrons

Location of Nonmetals on Periodic Table

Right side of the periodic table

Diatomic Molecule

A molecule consisting of two atoms of the same element bonded together

Most Reactive Nonmetal

Fluorine

Noble Gases Reactivity

Noble gases do not react with other elements because they have a full 8 outer energy levels of electrons. They do not share, gain, or lose electrons

Metalloid Properties

Some properties of metals and some properties of nonmetals. Plus semiconductors.

Most Common Metalloid

Silicon

Key properties of Lithium

Alkali Metal Smallest atomic size Easily combines with nonmetals to form ionic compounds

Isotope

Atoms of the same element that have different numbers of neutrons.

Cation

A positively charged ion.

Anion

A negatively charged ion.

Valence Electron

An electron in the outermost energy level of an atom.

s-orbital electron capacity

2

p-orbital electron capacity

6

Charge of an atom

Determined by the ratio between the number of electrons and protons

Molecule

Two or more atoms held together by chemical bonds.

Compound

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

Subscript

A number written below and to the right of a chemical symbol in a formula, indicating the number of atoms of that element.

Coefficient

A number placed in front of a chemical formula in a balanced equation to indicate the number of molecules or moles of that substance.

Solubility

The ability of a substance to dissolve in a solvent.

Solvent

A substance that dissolves another substance.

Solute

A substance that is dissolved in a solvent.

Solution

A homogeneous mixture of two or more substances.

Pure Substance

A substance with a fixed chemical composition and distinct properties.

Homogeneous Mixture

A mixture in which the composition is uniform throughout.

Heterogeneous Mixture

A mixture in which the composition is not uniform throughout.

Mixture separation methods

Magnetic attraction, Filtration, evaporation, distillation

Ions interaction

Two positively charged ions will repel each other. Two oppositely charged ions will attract and form an ionic bond.

Element that loses electrons

Metals lose electrons, this would cause a positive charge and they are found on the left side of the periodic table.

Element that gains electrons

Nonmetals tend to gain electrons, this would cause a negative charge and they are found on the right side of the periodic table.

Covalent bond

During Covalent bonding the electrons are being shared amongst two nonmetals. During ionic bonding the electrons are being gained or lost between a metal and nonmetal.

Elements in covalent bonds

Nonmetal and nonmetal

Chemical Change

Will change what the substance is.

Physical Change

Does not change the substance.

pH Scale ranges

0-7 Acid, 7 Neutral, 7-14 base

Acid Characteristics

Corrosive, sour, pH less than 7

Base Characteristics

Bitter, slipper/soapy, pH above 7

OH- Role in pH

A substance with an abundance of OH- will be more basic.

H+ Role in pH

A substance with an abundance of H+ will be more acidic.

pH Measurement Methods

Indicator solution, litmus paper, pH digital meter