Term
| The azimuthal quantum number is represented by what letter? |
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Definition
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Term
| Which of the following bond types are intermolecular? |
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Definition
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Term
| Which of the following bond types are intramolecular? |
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Definition
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Term
| The transition metals generally have one or two valence electrons. |
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Definition
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Term
| The nitrogen group has how many valence electrons? |
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Definition
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Term
| Which type of bond is formed by ionic solids dissolving in water? |
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Definition
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Term
| The spin quantum number is always represented by a negative number. |
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Definition
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Term
| Which bond type is formed between two polar molecules that contain hydrogen? |
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Definition
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Term
| Which of the following best defines the Pauli exclusion principle? |
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Definition
| C. No two electrons in an atom may have the same set of values for all four quantum numbers. |
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Term
| The spin quantum number is represented by what letter? |
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Definition
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Term
| Helium, an element with two valence electrons, is an exception to the eight valence electrons found in Group 18 elements. |
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Definition
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Term
| When moving from from one energy level to another, electrons emit photons. |
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Definition
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Term
| How many valence electrons do transition metals generally have? |
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Definition
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Term
| Which type of bond is formed by non-metals “stealing” electrons from metals? |
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Definition
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Term
| Which of the following best defines the Aufbau principle? |
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Definition
| B. An electron always tries to occupy the lowest possible energy state before filling higher states. |
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Term
| The alkaline earth metals are found in group 2 of the Periodic Table. |
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Definition
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Term
| Which of the following best defines Hund's rule of multiplicity? |
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Definition
| A. Only 1 electron will fill each orbital until each has an electron. After this, pairing will occur starting with the lowest energy states and working up to the higher states. |
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Term
| What is the term that defines the areas of electron density around a nucleus? |
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Definition
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Term
| What kind of orbital is a linear expansion of atomic orbitals? |
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Definition
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Term
| What is the maximum number of electrons that can be found in a d-shell? |
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Definition
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Term
| Van der Waals forces are predominant in polar-molecules. |
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Definition
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Term
| Which of the following is NOT a characteristic of ionic bonding? |
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Definition
| C. Ionic bonds have low electronegativity values. |
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Term
| Ionic bonds generally have high electronegativity differences. |
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Definition
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Term
| Which of the following best defines polymerization? |
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Definition
| B. The formation of molecular chains |
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Term
| Which type of interaction is involved in breaking ions out of the lattice by water molecules? |
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Definition
| C. Molecule-ion attraction |
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Term
| Which of the following is characteristic of covalent bonding? |
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Definition
| NOT NOT NOTB. Covalent bonding requires a highly electronegative non-metal bonding with a low electronegative metal. |
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Term
| Electronegativity decreases as you move up and across the Periodic Table from left to right. |
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Definition
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Term
| Which of the following is characteristic of metallic bonding? |
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Definition
| NOT NOT NOT A. Metallic bonds are formed from ionic bonds. |
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Term
| Which type of interaction is observable under non-standard conditions? |
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Definition
| NOT NOT NOT C. Ionic bonding |
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Term
| In hydrogen bonding, how many available lone valence electron pairs does oxygen have? |
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Definition
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Term
| Which of the following is characteristic of ionic bonding? |
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Definition
| A. Ionic bonds are formed between metals and non-metals. |
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Term
| Which type of interaction is involved in dissolving salt in water? |
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Definition
| C. Molecule-ion attractions |
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Term
| Covalent bonds are both polar and non-polar. |
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Definition
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Term
| Which of the following is characteristic of metallic bonding? |
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Definition
| NOT NOT NOT A. Metallic bonds are formed from ionic bonds. |
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Term
| Which type of interaction involves an induced dipole? |
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Definition
| C. Molecule-ion attractions NOT NOT NOT |
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Term
| Which of the following elements exhibits Van der Waals forces at non-standard conditions? |
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Definition
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Term
| How many potential water molecules can one water molecule bond to? |
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Definition
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Term
| Which of the following describes the charges on the atoms in a water molecule? |
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Definition
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Term
| Hydrogen bonding has a small degree of covalent characteristics. |
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Definition
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Term
| Which of the following is characteristic of covalent bonding? |
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Definition
| D. Covalent bonding is used in polymerization. |
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