CHM231- Day 1 Vocab
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Principal energy levels | (aka shells) region of space around a nucleus where electrons are found
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| Orbital | A region of space where an electron or pair of electrons spends 90 to 95% of its time
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| Ground-state electron configuration | The electron configuration of lowest energy for an atom, molecule, or ion
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| Valence electrons | Electrons in the valence (outermost) shell of an atom
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| Valence shell | The outermost electron shell of an atom in which valence electrons are found
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| Lewis structure of an atom | The symbol of an element surrounded by a number of dots equal to the number of electrons in the valence shell of an atom
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| Octet rule | The tendency among atoms in Group 1A-7A elements to react in ways that achieve an outer shell of eight valence electrons
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| Anion | An atom or group of atoms bearing a negative charge
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| Cation | An atom or group of atoms bearing a positive charge
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| Ionic bond | A chemical bond resulting from the electrostatic attraction of an anion and a cation
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| Covalent bond | A chemical bond resulting from the sharing of one or more pairs of electrons
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| Electronegativity | A measure of the force of an atom’s attraction for electrons it shares in a chemical bond with another atom
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| Bond length | The distance between the nuclei participating in a chemical bond
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| Nonpolar covalent bond | A covalent bond between atoms whose difference in electronegativity is less than approximately 1.5
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| Polar covalent bond | A covalent bond between atoms whose difference in electronegativity is betwee approximately 0.5 and 1.9
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| Dipole | In a [polar covalent bond?] A separation of charge between the more and less electronegative atoms in a molecular bond
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| Electron density model | A way to show electron density, with red (delta minus, δ-) being high and blue (delta plus, δ+) being low electron density
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| Bonding electrons | Valence electrons shared in a covalent bond
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| Nonbonding electrons | Valence electrons not involved in forming covalent bonds; that is, unshared electrons
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| Single bond | When two atoms share one pair of electrons
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| Double bond | When two atoms share two pairs of electrons
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| Triple bond | When two atoms share three pairs of electrons
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| Formal charge | The charge on an atom in a molecule or polyatomic ion (equation = valence electrons – (unshared electrons + ½ shared electrons))
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Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
To hide a column, click on the column name.
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You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
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