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Electron Configuration Part I

This segment examines ionization energy and explains the process for writing the electron configuration of any element.

Premiere Date: July 11, 2016 | Runtime: 00:04:09

Support Materials

Toolkit

Electron Configuration Cards
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Electron Configuration Chart
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Crosscutting Concepts

Patterns

Observed patterns of forms and events guide organization and classification, and they prompt questions about relationships and the factors that influence them.

Cause and Effect

Mechanism and explanation. Events have causes, sometimes simple, sometimes multifaceted. A major activity of science is investigating and explaining causal relationships and the mechanisms by which they are mediated. Such mechanisms can then be tested across given contexts and used to predict and explain events in new contexts.

Science & Engineering Practices

Generating a Hypothesis and Developing a Model

Modeling can begin in the earliest grades, with students’ models progressing from concrete “pictures” and/or physical scale models (e.g., a toy car) to more abstract representations of relevant relationships in later grades, such as a diagram representing forces on a particular object in a system. (NRC Framework, 2012, p. 58)

Vocabulary

anion - a negatively charged ion.

atomic number - the number of protons in the nucleus of an atom. 

atomic radius - the distance from the atom's nucleus to the outermost energy level. 

average atomic mass - a weighted average of all of the isotopes of that element in the universe. 

cation - a positively charged ion. 

effective nuclear charge (Zsubeff) - the net positive charge experienced by the valence electrons from the nucleus. 

electron - a tiny particle with a negative charge that is found outside the nucleus of an atom. 

electron configuration - the order in which electrons are arranged in an atom. 

electronegativity - the ability of an atom to attract additional electrons. 

energy sublevel - a smaller part within a primary energy level. 

excited state - an atom, ion or molecule with an electron in a higher than normal energy level than its ground state. 

ground state - the lowest energy state within electron orbitals. 

Hund's Rule - When placing electrons in equal energy orbitals, electrons should not be paired until each equal energy orbital contains one electron. 

ion - an atom with a positive or negative charge. 

ionization energy - the amount of energy required to remove one valence electron from an atom.

isotope - the same element with different numbers of neutrons.

model - a physical, conceptual, or mathematical representation of a real phenomenon whose purpose is to explain and predict the observed phenomenon. 

orbital - a region of space around the nucleus of an atom where an electron is likely to be found. 

Pauli exclusion principle - when an orbital holds two electrons, the electrons much have opposite spin. 

quantum - a specific amount of energy that can be absorbed by an electron as it moves from ground state to excited state, or released by an electron as it falls from the excited state back to ground state. 

subatomic- any smaller part of an atom such as a proton, neutron, or electron. 

valence electrons - electrons on the outer-most energy level of any atom. 

valence shell - the outer-most energy level of an electron. 

Georgia Standards of Excellence

SC1.fUse the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms (including atomic radii, ionization energy, and electronegativity of various elements).

SC1.gDevelop and use models including electron configuration of atoms and ions to predict an element’s chemical properties.

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