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Chem Exam 2
Sections 3.3-6.2, based on class content
| Question | Answer |
|---|---|
| What is an atomic orbital? | Region in an atom not in the nucleus where an electron is most likely to be |
| What is the purpose of quantum numbers? | Used to determine the electron configuration of an atom and the location of its electrons |
| What are the four quantum numbers? | m, l, m sub l, m sub s |
| What does the first quantum number refer to? | Energy level of the electron |
| What does the second quantum number refer to? | Shape of the orbital |
| What does the third quantum number refer to? | Orientation of the orbital |
| What does the fourth quantum number refer to? | Spin of the electron |
| What is not allowed in terms of the quantum numbers? | No two electrons can have the same four numbers |
| What is Hund's rule? | Everybody gets one before someone gets two |
| What is Aufbau? | Fill the lowest energy level first |
| What is a covalent radius? | One half the distance between the nuclei or identical atoms |
| What is effective nuclear charge? | Pull on a specific electron by the nucleus influenced by electron-electron interactions |
| What is shielding? | Blocking of valence electron attraction by the nucleus |
| What happens to atomic radius as you travel down the periodic table? | Gets bigger |
| What happens to atomic radius as you travel right across the periodic table? | Gets smaller |
| What is an ionic radius? | Distance from nucleus to edge of the electron cloud for an ion |
| What is the relationship between an atom and its cation's radius? | Cation is smaller |
| What is the relationship between an atom and its anion's radius? | Anion is bigger |
| What does it mean to be isoelectronic? | Same amount of electrons, same electron configuration |
| What is ionization energy? | Amount of energy required to remove an electron |
| What is second ionization energy? | Amount of energy required to remove a second electron |
| What happens to ionization energy as you travel down the periodic table? | Energy goes down |
| What happens to ionization energy as you travel right across the periodic table? | Energy goes up |
| What group will always have high ionization energies? | Noble Gases |
| Where are metals on the periodic table? | Left side |
| Where are nonmetals on the periodic table? | Right side |
| Where does most chemistry happen in the periodic table? | s and p groups |
| What is an ionic bond? | Electron transfer where the charges hold the atoms together |
| What is a covalent bond? | Electron is shared between two atoms forming a bond |
| What elements form an ionic bond? | Metal and nonmetal |
| What elements form a covalent bond? | Nonmetal and nonmetal |
| How can you tell the difference between an "ite" polyatomic ion and an "ate" polyatomic ion? | "Ite" has one less oxygen than "ate" |
| What does an "ite" ion turn into? | "Ous" acid |
| What does an "ate" ion turn into? | "Ic" acid |
| What electronegativity results in a nonpolar bond? | Less than 0.4 difference |
| What electronegativity results in a polar bond? | 0.5-1.7 difference |
| What electronegativity results in an ionic bond? | Greater than 1.8 difference |
| How do you name an ionic compound? | Name metal, name nonmetal, change ending to "ide" |
| How do you name a covalent compound? | Name nonmetal one, name nonmetal two, change ending to "ide," add prefixes |
| What does a roman numeral in a compound tell you? | Charge of the metal |
| In a binary compound, how do you name an aqueous acid? | Hydro, element, "ic" acid |
| In a non-binary compound, how do you name an aqueous acid? | Same rules as ions, determine charges based on how many Hydrogen atoms are present |
| What is a Lewis dot structure? | Elemental symbol surrounded by one dot for each valence electron |
| When is it ok to expand an octet? | Elements in the third row or below |
| What is formal charge? | Valence electrons-number of unbonded electrons-number of bonds |
| What is the ideal formal charge? | 0 |
| What is resonance? | Multiple legal and equivalent Lewis structures |
| What is the ideal bond angle for a linear molecule? | 180 |
| What is the ideal bond angle for a trigonal planar molecule? | 120 |
| What is the ideal bond angle for a tetrahedral molecule? | 109.5 |
| What is the ideal bond angle for a trigonal bipyramidal molecule? | 120 and 90 |
| What is the ideal bond angle for an octahedral molecule? | 90 |
| What is a trigonal planar geometry with one lone pair called? | Bent |
| What is a tetrahedral geometry with one lone pair called? | Trigonal pyramidal |
| What is a tetrahedral geometry with two lone pairs called? | Bent |
| How do you get delocalization? | In a resonant structure, electron jumps between possible places |
| What are the four types of orbitals? | s, p, d, f |
| What do we call the first type of connection between molecular orbitals? | Sigma bonds |
| Where are sigma bonds located? | Internuclear space |
| What do we call the second type of connection between molecular orbitals? | Pi bonds |
| Where are pi bonds located? | Side overlap of orbitals |
| What are the five hybridized orbitals we talked about in class? | sp, sp2, sp3, sp3d, sp3d2 |
| Are pi bonds found in hybridized orbitals? | No, they are in singly unoccupied p orbitals left over after hybridization |
| What kinds of molecules will we use in MO diagrams? | Diatomic |
| How do you calculate bond order? | Good bonds-bad bonds/2 |
| What does it mean to be paramagnetic? | There are some unpaired electrons |
| What does it mean to be diamagnetic? | There are no unpaired electrons |
| What do we think of free radicals? | BAD |
| What is formula mass? | Sum of the average atomic masses of all the atoms in the formula |
| Why do ionic compounds not exist as molecules? | The empirical formula is the only formula |
| How do you create an empirical formula? | Convert mass to moles, divide by smallest number of moles, then multiply to get all integers |
| How do you get percent compositions? | Divide mass of the element by mass of the compound |
| What names can ionic compounds use for mass? | Formula mass, molar mass |
| What names can molecular compounds use for mass? | Molecular mass, molar mass |
Created by:
gymnasticat
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