Electronic Structure of Atoms

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23 Terms

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<p>Continuous Line Spectrum</p>

Continuous Line Spectrum

When light passes through a prism it splits to give a continuous spectrum

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<p>Emission Line Spectrum</p>

Emission Line Spectrum

Light is passed through a hot sample of gas. The emission line spectrum represents the light emitted by an atom when its electrons fall back to lower energy levels.

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<p>Absorption Line Spectrum</p>

Absorption Line Spectrum

Light is passed through a cold sample of gas. The missing colours represent energy that entered the atom taken in by electrons.

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Energy Level

The fixed energy value that an electron in an atom may have

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Ground State of an Atom

One in which the electrons occupy the lowest available energy level

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Excited State of an Atom

One in which the electrons occupy higher energy levels than those available in the ground state

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Neils Bohr

Suggested the lines on the emission line spectrum represent energy levels with in an atom where electron could be found revolving around the nucleus in orbits

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Photon of light explanation

In its ground state, electrons occupy the lowest available energy level. The electron can move (jump/become excited) to a higher energy level if it receives a certain amount of energy. The excited state is unstable and the electron falls back to a lower level. It emits the excess energy in the form of a photon of light.

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Limitations to Bohr’s theory

Bohr’s theory only worked to explain the emission spectrum of Hydrogen.Bohr’s theory did not take into account the fact that an electron had a wave motion. Did not take into account the presence of sublevels.

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Sublevel

A a subdivision of a main energy level and consists of one or more orbitals of the same energy

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Atomic Orbital

A region in space where there is a high probability of finding an electron

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De Broglie

Stated that all moving particles move in wave motion

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Heisenberg’s Uncertainty Principle

Its not possible to determine the exact position and speed of an electron at the same time only the possibility of locating an electron in a given place at any one time

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Schrödinger

Developed a complex equation to calculate the location of an electron at any place at any one time. This equation revealed energy sublevels contain orbitals

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Aufbau Principle

Electrons will occupy the lowest available energy sublevel

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Hund’s Rule of Maximum Multiplicity

When two or more orbitals of equal energy are available, the electrons occupy them singly before filling them in pairs.

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Pauli Exclusion Principle

No more than 2 electrons may occupy an orbital and they must have opposite spin.

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Flame Tests: Sodium (Na)

Yellow

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Flame Tests: Potassium (K)

Lilac

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Flame Tests: Lithium (Li)

Crimson

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Flame Tests: Copper (Cu)

Blue-green

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Flame Tests: Barium (Ba)

Green

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Flame Tests: Strontium (Sr)

Red