Term
| What is the mutual electrical attraction between the nuclei and valence electrons of different atoms that bind the atoms together? |
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Definition
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Term
| Why do atoms bond together? |
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Definition
| To stabilize the valence shell and to decrease energy |
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Term
| What type of bond results from the electrical attraction between charged atoms? |
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Definition
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Term
| What will be the difference in electronegativiy between the atoms involved in an ionic bond? |
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Definition
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Term
| What is the term given to the positive ion? |
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Definition
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Term
| What is the term given to the negative ion? |
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Definition
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Term
| What type of bond results from the sharing of electrons? |
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Definition
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Term
| What are the two types of covalent bonds? |
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Definition
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Term
| What type of covalent bond shares the electrons equally? |
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Definition
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Term
| What type of covalent bond does not share the electrons equally? |
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Definition
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Term
| What is the difference in electronegativity between the two atoms involved in a nonpolar covalent bond? |
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Definition
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Term
| What is the difference in electronegativity between two atoms in a polar covalent bond? |
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Definition
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Term
| What is the term used to describe the ability of an atom to attract electrons? |
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Definition
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Term
| What is the neutral group of atoms that are held together by covalent bonds? |
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Definition
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Term
| Describe the importance of a chemical formula |
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Definition
| Chemical formulas indicate the relative numbers of atoms in each chemical compound |
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Term
| What types of atoms are bonding to form a molecule? |
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Definition
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Term
| How many diatomic atoms are there? What are the names of them? |
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Definition
| 7- H2, O2, N2, F2, Cl2, Br2, and I2 |
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Term
| Describe the formation of a covalent bond |
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Definition
| Two nonmetals share electrons to fill both of their outermost energy levels |
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Term
| As bond length decreases in covalent bond, what happens to the strength (bond energy) |
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Definition
| It increases because the shorter the bond length, the harder it is to break |
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Term
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Definition
| Chemical compounds tend to form so that each atom has an octet of electrons in their highest energy level |
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Term
| Give 4 exceptions of the octet rule |
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Definition
Beryllium-4 valence
Boron-6 valence
Phosphorus-10 valence
Sulfur-12 valence
Hydrogen-2 valence |
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Term
| What is the name given to the unshared pair of electrons in a lewis structure? |
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Definition
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Term
| What is the difference between a lewis structure and a structural formula? |
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Definition
| Lewis structures show electron dot pairs while structural formulas show don't show unshared pairs |
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Term
| What type of covalent bond involves the sharing of 1 pair of electrons? 2 pairs? 3 pairs? |
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Definition
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Term
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Definition
| The simplest collection of atoms from which an ionic compound's formula can be established |
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Term
| What is the relationship between ionic bond strength and lattice energy? |
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Definition
| Bond strength increases as lattice energy becomes more negative |
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Term
| NaCl and Al2O3 are both examples of (ionic/covalent) bonds |
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Definition
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Term
| (ionic/covalent) bonds have low melting and boiling points |
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Definition
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Term
| (ionic/covalent) bonds are conductors in water |
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Definition
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Term
| (ionic/covalent) bonds are a network of + and - ions |
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Definition
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Term
| (ionic/covalent) bonds are hard and brittle solids |
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Definition
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Term
| (ionic/covalent) bonds are non-conductors in water |
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Definition
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Term
| H2O and CO2 are examples of (ionic/covalent) bonds |
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Definition
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Term
| What is a polyatomic ion? |
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Definition
| A charged group of covalently bonded atoms |
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Term
| What is the term used to describe the electrons of metals? |
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Definition
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Term
| What does "delocalized" mean? |
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Definition
| Electrons do not belong to any one atom |
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Term
| Because they don't belong to any one atom, what phrase describes a metal's electrons? |
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Definition
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Term
| What are some properties of metals? |
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Definition
| High electrical and thermal conductivity, luster, malleable, and ductile |
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Term
| Why do metals have luster? |
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Definition
| Metals absorb light and re-radiate this light in a frequency similar to the absorbed frequency |
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Term
| What is the relationship between enthalpy of vaporization and the bond strength of metals? |
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Definition
| The stronger the bond, the greater the enthalpy of vaporization |
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Term
Molecular shape: linear
Name the bond angle, # of atoms bonded to central atom, and # of lone pairs of electrons |
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Definition
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Term
Molecular shape: trigonal planar
Name the bond angle, # of atoms bonded to central atom, and # of lone pairs of electrons |
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Definition
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Term
Molecular shape bent or angular:
Name the bond angle, # of atoms bonded to central atom, and # of lone pairs of electrons |
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Definition
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Term
Molecular shape tetraheadral:
Name the bond angle, # of atoms bonded to central atom, and # of lone pairs of electrons |
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Definition
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Term
Molecular shape trigonal pyramidal:
Name the bond angle, # of atoms bonded to central atom, and # of lone pairs of electrons |
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Definition
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Term
Molecular shape bent or angular with 2 lone pairs:
Name the bond angle, # of atoms bonded to central atom, and # of lone pairs of electrons |
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Definition
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Term
Molecular shape trigonal bipyramidal:
Name the bond angle, # of atoms bonded to central atom, and # of lone pairs of electrons |
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Definition
| 90 and 120 degrees, 5, 0. |
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Term
Molecular shape octaheadral:
Name the bond angle, # of atoms bonded to central atom, and # of lone pairs of electrons |
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Definition
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Term
| What does V.S.E.P.R. stand for? |
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Definition
| Valence Shell Electron Pair Repulsion |
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Term
| What is a hybrid orbital? |
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Definition
| Orbitals of equal energy produced by the combination of two or more orbitals on the same atoms |
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Term
| What are the three types of intermolecular forces? |
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Definition
Dipole-dipole- two polar molecules
Hydrogen bonding-occurs between H and F, O, or N
London dispersion-two nonpolar molecules |
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Term
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Definition
| Substances that have the same molecular formula as another substance but differ in structure |
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Term
| Name four types of isomers |
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Definition
| Structural, geometric, positional, functional |
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Term
| What happens in structural isomers? |
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Definition
| The carbon chain is altered |
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Term
| What happens in geometric isomers? |
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Definition
| They differ in the arrangement around double bonds |
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Term
| What happens in positional isomers? |
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Definition
| They differ in position of double bond or atom other than C or H |
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Term
| What happens in functional isomers? |
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Definition
| An element other than C or H is bonded in a different way |
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Term
The hybrid sp:
Name the # of orbitals produced, bond angle, and basic shapes |
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Definition
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Term
The hybrid sp2:
Name the # of orbitals produced, bond angle, and basic shapes |
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Definition
| 3, 120 degrees, trigonal planar. |
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Term
sp3 hybrid:
Name the # of orbitals produced, bond angle, and basic shapes |
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Definition
| 4, 109.5 degrees, tetraheadral |
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