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CHM231- Day 1 Vocab
| Question | Answer |
|---|---|
| Principal energy levels | (aka shells) region of space around a nucleus where electrons are found |
| Orbital | A region of space where an electron or pair of electrons spends 90 to 95% of its time |
| Ground-state electron configuration | The electron configuration of lowest energy for an atom, molecule, or ion |
| Valence electrons | Electrons in the valence (outermost) shell of an atom |
| Valence shell | The outermost electron shell of an atom in which valence electrons are found |
| 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 |
| Octet rule | The tendency among atoms in Group 1A-7A elements to react in ways that achieve an outer shell of eight valence electrons |
| Anion | An atom or group of atoms bearing a negative charge |
| Cation | An atom or group of atoms bearing a positive charge |
| Ionic bond | A chemical bond resulting from the electrostatic attraction of an anion and a cation |
| Covalent bond | A chemical bond resulting from the sharing of one or more pairs of electrons |
| Electronegativity | A measure of the force of an atom’s attraction for electrons it shares in a chemical bond with another atom |
| Bond length | The distance between the nuclei participating in a chemical bond |
| Nonpolar covalent bond | A covalent bond between atoms whose difference in electronegativity is less than approximately 1.5 |
| Polar covalent bond | A covalent bond between atoms whose difference in electronegativity is betwee approximately 0.5 and 1.9 |
| Dipole | In a [polar covalent bond?] A separation of charge between the more and less electronegative atoms in a molecular bond |
| 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 |
| Bonding electrons | Valence electrons shared in a covalent bond |
| Nonbonding electrons | Valence electrons not involved in forming covalent bonds; that is, unshared electrons |
| Single bond | When two atoms share one pair of electrons |
| Double bond | When two atoms share two pairs of electrons |
| Triple bond | When two atoms share three pairs of electrons |
| 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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