ICPS Spring Final (Unit 5-12)

Coulomb's Law

Describes the force between two charged particles.

Electrostatic Force (Fe)

The force calculated using Coulomb's Law: Fe = k(Q1*Q2)/d^2.

k (Coulomb's constant)

Constant used in the calculation of electrostatic force.

Charge (Q)

The electrical property of matter responsible for attraction and repulsion.

Attractive Forces

Forces that pull charged particles towards each other.

Repulsive Forces

Forces that push charged particles away from each other.

Units of Charge

Measured in Coulombs (C).

Distance in Coulomb's Law

Measured in Meters (m); distance between objects affects the force between them.

Electrons

Negatively charged subatomic particles.

Protons

Positively charged subatomic particles.

Neutrons

Neutral subatomic particles found in the nucleus.

Atomic Nucleus

Small, dense region at the center of an atom containing protons and neutrons.

Electron Cloud

Area around the nucleus where electrons are likely to be found.

Isotopes

Atoms of an element with a different number of neutrons.

Cations

Positively charged ions formed by the loss of electrons.

Anions

Negatively charged ions formed by the gain of electrons.

Ionic Bonding

Chemical bond formed by the attraction between cations and anions.

Molar Mass

Amount of grams in 1 mole of a substance.

Avogadro's Number

6.022 x 10^23 particles in 1 mole of a substance.

Balancing Chemical Equations

Making sure the number of each type of atom is equal on both sides of a chemical equation.

Stoichiometry

The relationship between quantities of reactants and products in a chemical reaction.

Endothermic Reactions

Reactions that absorb heat from the surroundings.

Exothermic Reactions

Reactions that release heat to the surroundings.

Second Law of Thermodynamics

The entropy of the universe is always increasing.

Entropy (S)

A measure of randomness or disorder in a system.

Heat Transfer

The movement of thermal energy from one object to another.

Specific Heat Capacity

The amount of heat required to raise the temperature of 1 gram of a substance by 1°C.

Coulomb's Law

Describes the force between two charged particles.

Electrostatic Force (Fe)

The force calculated using Coulomb's Law: Fe = k(Q1*Q2)/d^2.

k (Coulomb's constant)

Constant used in the calculation of electrostatic force.

Charge (Q)

The electrical property of matter responsible for attraction and repulsion.

Attractive Forces

Forces that pull charged particles towards each other.

Repulsive Forces

Forces that push charged particles away from each other.

Units of Charge

Measured in Coulombs (C).

Distance in Coulomb's Law

Measured in Meters (m); distance between objects affects the force between them.

Electrons

Negatively charged subatomic particles.

Protons

Positively charged subatomic particles.

Neutrons

Neutral subatomic particles found in the nucleus.

Atomic Nucleus

Small, dense region at the center of an atom containing protons and neutrons.

Electron Cloud

Area around the nucleus where electrons are likely to be found.

Isotopes

Atoms of an element with a different number of neutrons.

Cations

Positively charged ions formed by the loss of electrons.

Anions

Negatively charged ions formed by the gain of electrons.

Ionic Bonding

Chemical bond formed by the attraction between cations and anions.

Molar Mass

Amount of grams in 1 mole of a substance.

Avogadro's Number

6.022 x 10^23 particles in 1 mole of a substance.

Balancing Chemical Equations

Making sure the number of each type of atom is equal on both sides of a chemical equation.

Stoichiometry

The relationship between quantities of reactants and products in a chemical reaction.

Endothermic Reactions

Reactions that absorb heat from the surroundings.

Exothermic Reactions

Reactions that release heat to the surroundings.

Second Law of Thermodynamics

The entropy of the universe is always increasing.

Entropy (S)

A measure of randomness or disorder in a system.

Heat Transfer

The movement of thermal energy from one object to another.

Specific Heat Capacity

The amount of heat required to raise the temperature of 1 gram of a substance by 1°C.

Democritus's Model

Everything is made up of physically indivisible & indestructible atoms. Empty space exists between atoms. Atoms are in perpetual motion. Infinite number and types of atoms (e.g size & shape)

Dalton's Model

Matter is made up of indivisible & indestructible atoms. All atoms of an element are identical (in mass & chemical properties). Atoms of different elements combine in simple whole numbers to form compounds. A chemical reaction is a rearrangement of atoms.

Thomson's Plum Pudding Model

Electrons & some positively charged matter compose atoms

Rutherford's Model

Small, dense, positively charged nucleus in the center of the atom. Tiny electrons circling the nucleus.

Bohr's Model

Electrons can only exist at specific energy levels and not in between. The higher the shell number, the greater the energy of electrons in that shell. Electrons can move up shells when energy is gained and move down to lose energy

Quantum Model

Electrons are likely found in the electron cloud. Electron are most likely to be found in the most dense areas of the electron cloud (also the region of their orbital). Shows probability functions for where an electron can be found

Democritus Model

Everything is made up of physically indivisible & indestructible atoms. Empty space exists between atoms. Atoms are in perpetual motion. Infinite number and types of atoms (e.g size & shape)

Dalton's Model

Matter is made up of indivisible & indestructible atoms. All atoms of an element are identical (in mass & chemical properties). Atoms of different elements combine in simple whole numbers to form compounds. A chemical reaction is a rearrangement of atoms.

Thomson's Plum Pudding Model

Electrons & some positively charged matter compose atoms. Experiment: Cathode Ray Tube (1904): In a vacuum within a sealed glass tube (air is evacuated), a beam of electricity is shot through the tube, appearing as a ray of particles. Two oppositely charged plates are placed around the cathode ray, and the ray is deflected from the negatively charged plate and towards the positively charged plate. What did the Experiment Prove?: Based on how much the cathode ray bent, particles smaller than atoms must exist. The particles are negatively charged. Some positively charged matter must exist within an atom (something positive must balance out the negative electrons because most matter is neutral).

Rutherford's Model

Small, dense, positively charged nucleus in the center of the atom. Tiny electrons circling the nucleus. Experiment: Gold Foil Experiment (1911): Alpha particles (positively charged; composed of 2 protons & 2 neutrons) are shot at a thin piece of gold foil. Alpha particles were expected to all pass through the foil as an atom was theorised to be empty space and electrons (extremely small). Some alpha particles were surprisingly deflected. What did the Experiment Prove?: Disproved Plum Pudding Model. Proved there must be some small, dense, positive mass in the center of the atom that is deflecting the positive alpha particles.

Bohr's Model

Electrons can only exist at specific energy levels and not in between. The higher the shell number, the greater the energy of electrons in that shell. Electrons can move up shells when energy is gained and move down to lose energy. Experiment: Bohr used past experiments to develop and support his model: Atomic Emission Spectra: each element glows a distinct color when an electric current is passed through it, suggesting various atoms only emit certain wavelengths of light. Quantum Theory: every physical body can emit or absorb energy in distinct amounts in the form of electromagnetic radiation. What did the Experiment Prove?: Bohr suggested atomic spectrum is made by electrons moving between energy levels. Electrons exist at distinctive energy levels, also called shells.

Quantum Model

Electrons are likely found in the electron cloud. Electron are most likely to be found in the most dense areas of the electron cloud (also the region of their orbital). Shows probability functions for where an electron can be found