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33 Cards in this Set
- Front
- Back
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What are the 7 groups in the periodic table? |
Alkali metals, halogens, transition elements, lanthanides, alkaline-earth metals, noble gases, and actinides. |
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What are the trends in reactivity within the periodic table? |
- Metals in the bottom left corner are the most reactive. - Nonmetals in the upper right corner are the most reactive. - Noble gases are considered non-reactive. |
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What are valence electrons? |
Electrons occupying the highest energy level of an atom. |
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What are bonding electrons? |
Unpaired electrons that are involved in bond formation. |
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What are lone pairs? |
Paired electrons that are generally not involved in bond formation. |
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What is electronegativity? |
The term is used to describe the relative ability of an atom to attract a pair of bonding electrons in its valence level. |
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What is an orbital? |
A region in space in which an electron with a given energy is likely to be found. |
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What is the Lewis model? |
A model of the distribution of electrons in valence orbitals. Includes the chemical symbol of an element and dots to represent the valence electrons. |
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What is an ionic bond? |
An ionic bond is the attraction that results from a positive ion and a negative ion, in which a transfer of electrons occurs. |
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What is a positive ion? |
A positive ion is formed when an atom loses electrons to become similar to the nearest noble gas. |
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What is a negative ion? |
A negative ion is formed when an atoms gains electrons to become similar to the nearest noble gas. |
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What is a covalent bond? |
The bond that results from the electrostatic attraction between the electrons of one atom to the nucleus of another and vice versa. |
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Malleable & Ductile |
The layers of metallic ions can slide past each other without the need to break. |
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Conducts electricity |
The delocalized electrons are free to move from one side of the lattice to the other. They can carry a current. |
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High Melting Point |
The more electrons that are donated to the sea of electrons, the stronger the positive charge of the cations. This leads to a greater attraction to the electron sea and the the melting/boiling point. |
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What are metalloids? |
The elements along the staircase of the periodic table have both properties of metals and nonmetals. |
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Molecular compounds |
Form covalent bonds (electrons are shared) |
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What are double bonds? |
When two atoms share two pairs of electrons |
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What are triple bonds? |
When two atoms share three pairs of electrons. These bonds con occur between nonmetals. |
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What is a dative bond? |
A bond where both electrons originate from the same atoms. |
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What are hybrid diagrams? |
A diagram in which all electron pairs are displayed. |
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Molecular formula? |
Shows the actual number of atoms of each element in a molecule. |
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Empirical Formula |
The simplest whole number ratio of atoms of each element in a particle of a substance. |
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VSEPR |
Valence Shell Electron Pair Repulsion Theory |
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VSEPR Definition |
Pairs of electrons arrange themselves around the central atom so that they are as far apart from each other as possible. This results in molecules having specific shapes. |
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Negative charge centers |
An area that contains at least 1 pair of electrons (areas of high electron density) |
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Polarity |
A polar molecule is a molecule that has an overall charge separation. |
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Intermolecular forces |
The weak forces or bonds among molecules |
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Intramolecular bonds |
Attractions within a molecule |
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Intermolecular bonds |
Involve the electrostatic attractive forces between molecules |
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London Dispersion Forces |
This weak attractive force results when the electrons of one molecule are attracted to the positive nuclei of a nearby molecule. |
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Dipole-Dipole Forces |
If the substance contains polar molecules the the positive end of one molecule will be attracted to the negative end of a neighboring molecule, this will extend in all directions. |
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Hydrogen Bonding |
Occurs when hydrogen is bonded to a highly electronegative element. |
