Atomic Structure and Electron Configuration: Chemistry for Changing Times, Chapter 3

Electrolysis

The chemical reactions caused by electricity.

Ions

Charged atoms (or groups of atoms).

Cation

Positively charged ion.

Electrolyte

A compound that conducts electricity when melted or put into solution.

Cathode rays

Beams of electrons.

Mass of the electron

Determined by measuring the deflection of cathode rays in electrical and magnetic fields.

Charge on the electron

Determined by measuring the deflection of cathode rays in electrical and magnetic fields.

Ratio of mass to charge for the electron

Determined by measuring the deflection of cathode rays in electrical and magnetic fields.

Humphry Davy

A scientist grouped with others for the application of electricity to chemical systems.

Michael Faraday

A scientist grouped with others for the application of electricity to chemical systems.

J.J. Thomson

A scientist grouped with others for the application of electricity to chemical systems.

Ernest Rutherford

A scientist NOT grouped with others for the application of electricity to chemical systems.

Qualitative observations

Provide glimpses of the structure of matter influenced by ideas related to magic and mysticism.

Quantitative measurements

Lead to the formulation of fundamental laws leading to an atomic theory of matter.

Electricity

Played an important role in unraveling the structure of the atom.

Experimental evidence

Provided for the existence of subatomic particles through the application of electricity to chemical systems.

Subatomic particles

Constituents of all matter speculated from observations of cathode rays.

Electrodes

Not defined in the context of the provided notes.

Neutrons

Not defined in the context of the provided notes.

Protons

Not defined in the context of the provided notes.

Experimental observation of cathode rays

The rays were independent of the type of gas in the vacuum tube.

First experimental verification of positively charged particles

Goldstein.

Millikan's oil drop apparatus

Allowed for the determination of the charge of the electron.

Combined findings of Millikan and Thomson

Allowed for the determination of the mass of the electron.

Anion

Negatively charged ion.

Cathode ray

A beam that seemed to leave the cathode and travel to the anode.

Effect of magnetic field on a stream of electrons

The stream would be deflected toward the positive electrode.

Cathode

Negative electrode.

Anode

Positive electrode.

Radioactivity

The spontaneous emission of radiation from unstable elements.

Marie Sklodowska Curie

The person who won two Nobel prizes (one in physics; the other in chemistry) for work with radioactivity.

Fluorescence

The phenomenon where some chemicals exposed to sunlight continue to glow even when placed in a dark room.

He2+ particle

Symbolized by He2+, it is identified as alpha, α.

Least penetrating particle

The alpha particle, α, is the least penetrating.

Electromagnetic radiation from unstable elements

Gamma rays are emitted from unstable elements.

Non-radioactive particle type

Lambda, λ is NOT one of the three types of radiation emitted from radioactive elements.

Radioactivity not deflected by magnetic field

Gamma, γ is NOT deflected by a magnetic field.

Positive charge particle

Alpha, α has a positive charge.

Negative charge particle

Beta, β has a negative charge.

Electron particle

Beta, β is identified as an electron.

alpha, α

A type of radioactivity that has mass.

beta, β

A type of radioactivity that has mass.

gamma, γ

A type of radioactivity that has essentially no mass.

lambda, λ

Not a type of radioactivity.

Geiger and Marsden experiments

Experiments that used alpha particles with thin metal foils.

nuclear model of the atom

Constructed from the alpha particle scattering experiment.

Rutherford's proposal

Atoms are mostly empty space, with most mass in a dense nucleus.

nucleus of an atom

Composed of protons and neutrons packed tightly into a very small volume.

positively charged nucleus

Concluded by Rutherford due to deflection of positively charged alpha particles.

critical thinking skills

Ability to think critically and analyze information.

types of radiation

Alpha, beta, and gamma are the three main kinds.

deflection by magnetic field

Alpha and beta particles are deflected, gamma is not.

Rutherford

Proposed the nuclear model of the atom.

Dalton

Not associated with the nuclear model of the atom.

Thomson

Not associated with the nuclear model of the atom.

Millikan

Not associated with the nuclear model of the atom.

nuclear physicists

Have discovered over 100 different particles that compose the nucleus.

positively charged alpha particles

Deflected by the nucleus in the gold foil experiment.

negatively charged beta particles

Not deflected by the nucleus in the gold foil experiment.

gold foil experiment

An experiment that demonstrated the nuclear nature of the atom.

atomic spectra

Not the fundamental experiment for the nuclear model.

cathode ray behavior

Not the fundamental experiment for the nuclear model.

electrolysis of water

Not the fundamental experiment for the nuclear model.

Difference in mass between protons and neutrons

Insignificant.

Mass of an atom

Essentially all of the mass of an atom is due to nucleons.

Mass of electrons in atoms

Generally regarded as insignificant.

Mass of a nucleon

1 atomic mass unit (u).

Comparison of isotopes' properties

Isotopes generally have the same chemical properties, but often different nuclear properties.

Charge on the nucleus of a sodium atom

11+.

Isotopes of iron (Fe)

Each of these isotopes has 26 protons, 26 electrons, and a different number of neutrons.

Sum of protons and neutrons in an atom

Nucleon number.

Neutrons in an isotope of tin (Sn)

66.

Nucleons in an isotope of calcium (Ca)

46.

Nucleons

Particles that make up the nucleus of an atom.

Carbon-14

An isotope of carbon commonly referred to as 'carbon-14'.

Neutrons in Carbon-14

Carbon-14 contains 8 neutrons.

Neutrons in Sulfur-31

Sulfur-31 contains 16 neutrons.

Nucleons in Sulfur-35

Sulfur-35 contains 35 nucleons.

Phosphorus-31

The isotope P is also called phosphorus-31.

Uranium Isotope

The isotope identified as U.

Proton Mass and Charge

The proton has a larger mass and opposite charge compared to the electron.

Neutron Mass and Charge

The neutron has the same approximate mass as a proton, but no charge.

Tritium

Tritium is the common name for hydrogen-3.

Deuterium

Deuterium is the common name for hydrogen-2.

Nucleons in Tin Isotope

The isotope of tin contains 122 nucleons.

Neutrons in Nitrogen

Nitrogen contains 7 neutrons.

Neutrons in Boron

Boron contains 4 neutrons.

Neutrons in Silicon

Silicon contains 14 neutrons.

Isotope Identification

Identify elements and isotopes from their nuclear particles.

Quantitative Skills in Chemistry

Demonstrate the quantitative skills needed to succeed in chemistry.

Scientific Inquiry Principles

Demonstrate an understanding of the principles of scientific inquiry.

Isotope of Phosphorus

Phosphorus-31 is an isotope of phosphorus.

Isotope of Sulfur

Sulfur-35 is an isotope of sulfur.

Isotope of Uranium

Uranium is identified as U.

Isotope of Nitrogen

Nitrogen is identified as N.

Isotope of Boron

Boron is identified as B.

Neutron

the same approximate mass as a proton, but no charge.

Electron

the same approximate mass as an electron, but no charge.

Proton Discovery Timing

The experiment that confirmed the existence of neutrons was performed after the discovery of the proton.

Atomic Number

The number of protons in an atom.