Atomic Structure and Chemical Reactions Flashcards

Flashcards covering key vocabulary and concepts in atomic structure, chemical reactions, and stoichiometry.

Dalton’s theory

Atoms of different elements combine to form compounds in a fixed ratio.

Thomson model

Plum – pudding model.

Alpha particles

Positively charged helium nucleus.

Goldstein

Discovered protons.

Thomson

Discovered electrons.

Rutherford

Discovered the nucleus.

Chadwick

Discovered neutrons.

Gold foil

Rutherford fired alpha particles at this material.

Negative

Charge of electrons.

Positive

Charge of protons.

Zero

Charge of neutrons.

Protons and Neutrons

Particles in the nucleus.

Electrons

Particles outside the nucleus.

Atomic number

Fixed for an element.

Mass number

Number of protons and neutrons in an atom.

Atomic number

Number of protons and electrons.

Small

Size of the nucleus as compared to the size of an atom.

Cathode rays

Glowing beam from the cathode.

Anode

Positive electrode.

Cathode

Negative electrode.

Cathode rays

Made up of negatively charged particles and discovered electrons.

2n^2

Formula used to calculate the maximum number of electrons in an orbit.

s

Orbital with lowest energy and a sphere shape.

p

Orbital with energy greater than s-orbital and a dumbbell shape.

d

Orbital with energy greater than s and p-orbitals and a leaf shape.

f

Orbital with energy greater than d-orbitals and a complicated shape.

Valence Electrons

Electrons in the outermost shell

X-Rays

Waves used to penetrate solids and are used in doctor’s offices and airports.

Wavelength

Distance between one point of a wave to the same point in the next wave.

Frequency

Number of waves per unit of time.

Longitudinal Waves

Waves that occur when the motion of the medium is parallel to the direction of the wave.

Visible Light

Waves that have a color spectrum known as ROYGBIV.

Mechanical Waves

Waves that disturb matter.

Crest

Top of a wave.

Trough

Bottom of a wave.

Amplitude

Maximum distance that matter is displaced from the resting position.

Radio Waves

Waves produced by stars and galaxies.

Transverse Waves

Waves that occur when the motion of the medium is at right angles (perpendicular) to the direction of the wave.

Infrared Waves

Waves often used in heat lamps.

Ultraviolet Waves

Waves utilized by insects to locate nectar.

Electromagnetic Waves

Transverse waves that disturb electromagnetic fields.

Gamma Waves

Waves that have the shortest wavelength and the highest frequency.

Steel

Alloy made of Iron and Carbon.

Brass

Alloy made of Copper and Zinc.

Bronze

Alloy made of Copper and Tin.

Any free element

Has an oxidation number equal to zero.

monatomic ions

Oxidation number always has the same value as the net charge.

Hydrogen atom (H)

Exhibits an oxidation state of +1.

Oxygen

Has an oxidation of -2 in most of its compounds.

Alkali metals

Have an oxidation state of +1 in their compounds.

Alkaline earth metals

Exhibit an oxidation state of +2 in their compounds.

Halogen

Have an oxidation number of -1 assigned to them in compounds made up of two elements.

Ionic Compounds

Formed between metals and nonmetals.

Covalent Compounds

Formed between nonmetals.

Electronegativity

attraction tendency of an element to shared electrons

Polar Compounds

Different elements, no symmetry.

Nonpolar Compounds

Identical atoms, symmetry.

Decomposition

A type of chemical reaction: 2KClO3 ➝ 2KCl + 3O2

Combustion

A type of chemical reaction: 2C8H18 + 25O2 ➝ 16CO2 + 18H2O

Double Replacement

A type of chemical reaction: HNO3 + NaHCO3 ➝ NaNO3 + CO2 + H2O

Synthesis

A type of chemical reaction: Fe + O2 ➝ Fe2O3

Spectator Ions

Ions that do not participate directly in a chemical reaction and are present on both sides of the equation

Exothermic

When energy is released during reaction.

Endothermic

When energy is absorbed during reaction.

Acid

H+ (protons) ion donor.

Base

OH- (hydroxyl) ion donor.

of particles = moles × (6.02 × 10^23 particles/mole)

Formula for the number of particles.

Mole = [given particle] / (6.02 × 10^23 particles/mole)

Formula for calculating moles.

Mass(g) = Moles × MolarMass(g/mol)

Formula for calculating mass.

Moles = Mass(g) / MolarMass(g/mol)

Formula for calculating moles from mass.

Volume STP = Mole × 22.4 L/mol

Formula for volume at STP.

% of a substance = (Mass of the substance / Total Mass) × 100

Formula for percent composition.

Mole to Mole conversion

given moles × mole ratio