Atomic Structure Vocabulary

Vocabulary flashcards based on Atomic Structure lecture notes.

Matter

Any substance that occupies space and has mass.

Atom

Smallest particle of a substance that involves a chemical reaction; Simplest form in which an element can exist.

Atom

Simplest & neutral particle that can be divided into subatomic particles.

Democritus' Atomic Theory

States that matter is made of very small, invisible, indivisible particles called 'atoms'.

Dalton's Atomic Theory - Elements

Elements are made of atoms which are extremely small particles that cannot be divided further.

Dalton's Atomic Theory - Atomic Similarity

All atoms of an element are similar in mass and size, while atoms of different elements are different from each other.

Dalton's Atomic Theory - Atomic Conversion

Atoms of one element cannot be converted to an atom of another element by chemical reaction; Atoms can neither be created nor destroyed.

Dalton's Atomic Theory - Compound Formation

Two or more atoms of different elements combine in simple numerical ratios to form compounds.

Compound

A substance composed/made of two or more different elements.

Element

A substance made of two or more atoms of the same element.

Molecule

Made of one or more atoms of the same or different elements, bonded covalently and existing independently in nature (e.g., CO2, H2O).

Ions

Atoms or molecules that have an electrical charge due to the gain or loss of electrons (e.g., Na+, Cl-).

Atom (Modern Definition)

Smallest unit of an element that retains the element's chemical properties.

Electron

Basic particle of electricity, having material properties; Common to every matter.

Cathode Rays

Invisible particles emitted from the cathode in a vacuum tube when high voltage is applied.

Positive Rays/Anode Rays/Canal Rays

Proposed the existence of positive charges in matter; Observed in the positive ray experiment.

Anode Rays Characteristics

Positively charged particles that emerge near the anode and travel toward the cathode.

Hydrogen Ion (H+)

Positive ray with the lowest mass and highest charge-to-mass ratio.

Proton

Simplest positively charged particle, identified through positive ray experiments using hydrogen gas.

Radioactivity

Particles or waves emitted by unstable atomic nuclei in order to achieve stability.

Three Types of Radioactive Emissions

Alpha (α), Beta (β), and Gamma (γ).

Isotopes

Atoms with the same atomic number but different mass numbers; atoms with the same number of protons but different numbers of neutrons.

Mass Spectrograph

Instrument used to discover isotopes by filling it with Neon gas.

Chemical Properties of Isotopes

Number of electrons in isotopes is the same, and so are chemical properties (e.g. electronegativity, reactivity)

Physical Properties of Atom

Calculating average atomic mass and isotopes' mass numbers differ from each other (e.g. density).

Thomson's Plum Pudding Model

Proposed after discovery of electron to explain the structure of atom. Atom is a positively charged sphere in which negatively charged electrons are immersed/embedded.

Electromagnetic Waves

Waves that transmit energy through oscillating electric and magnetic fields perpendicular to each other.

Frequency (f)

Number of oscillations per unit time

Speed (V)

Distance a wave travels within a unit of time

Photons

Energy packets that electromagnetic waves transmit energy in; also known as 'Quanta'.

Wave Particle Duality of Electron

Electrons show wave properties in some instances. Exists in Super Position'

Particular Properties of Electrons

Electrons show wave properties in some instances. The ability to do work and charge.

Wave Properties of Electrons

Electrons show wave properties in some instances. Beams undergo refraction upon passage through narrow openings

De Broglie Equation

When a certain particle displays it's wave properties in order to calculate the wavelength.

E eins energy mass Equation

Equal amount of energy is released out and this equation displayes it

Absorption Spectrum

Spectrum formed when white light is flown through a prism, showing colours from red to purple.

Emission Spectrum

Spectrum obtained when electrical power is supplied to a bulb fitted with H2 gas, showing red, green, blue, and purple illumination on a dark background.

Energy Level Concept

Electrons stay around the nucleus in each energy levels and has the same energy values

Energy Level Concept- Electron Absorption

Electrons can absorb the energy and moves to higher energy levels

Energy Level Concept- Electron Emission

Energy level will emit energy and moved to lower energy levels

Energy Level Concept- Electron color

Always same colors that electron will absorb and emit

Excited State of Electrons

electrons jumps to higher energy levels because supplied to energy

Emission state of Energy

Electromagnetic Waves, that move to lower energy levels.

Series of Hydrogen Spectrum

Spectrum that are categorizes by electron movements (electron jump)

Lymen Series

When the electrons jump from the highest energy levels to 1st energy level

Lymen Spectrum- spectrum

spectrum are between 90nm-120nm, and belongs to UV range of electromagnetic spectrum

Balmer Series

When the Electron jump off to the 2ed energy level and higher

Balmer spectrum- spectrum

Line usually belong to the visible range/ uv range

Paschen series (IR)

When the electrons jump off to the 3rd energy level from higher energy level. range is 800km -300nm

Modern Atomic Structure- Nucleus

The positively charged nucleus exists in the middle of the atom

The first energy

level number is 1

The second energy

level number is 2

The third energy

level number is 3

Orbital Shapes

Electrons exists inside the atom as 'Orbitals', the region of electron can physically exists

Writing Quantam Numbers

electrons exists inside the atom, region name Orbitals

Principal Quantam Numbers (n)

The energy leve the election belongs to is presented

Angular Momentum Quantam Number (l)

The sub energy level that the electron belong to is described.

The Direction the electrons' spins 's'

Pauli Exclusion Principale

The Quantom Number

The Quanton electron

Inside orbital can be one of 2 electron

Pauli Exclusion Principale