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Exam 3
General Chemistry 1 Exam 3 Fall Semester 2025
| Question | Answer |
|---|---|
| What are quantum numbers used for? | Used to determine how electrons are arranged |
| What do quantum numbers determine? | Size, shape, and orientation in space of an orbital |
| What are the four types of quantum numbers? What variable is used to represent them? | Principal, n Angular momentum, l Magnetic, ml Spin, ms |
| What does the principal quantum number (n) determine and describe? | Determines size and energy Describes distance of the orbital from the nucleus |
| What does the angular momentum determine? What can the l values be? | Determines the shape l can be values from 0 to (n-1), values are represented by a particular level |
| If the value of l is 0, what (letter) orbital is it and what is the shape? | s spherical |
| If the value of l is 1, what (letter) orbital is it and what is the shape? | p two balloon tied at the knots |
| If the value of l is 2, what (letter) orbital is it and what is the shape? | d four balloons tied at the knots |
| If the value of l is 3, what (letter) orbital is it and what is the shape? | f eight balloon tied at knots |
| If the value of n is 1, what is the value of l and what sub shells are included? | 0 s |
| If the value of n is 2, what is the value of l and what sub shells are included? | 0, 1 s, p |
| If the value of n is 3, what is the value of l and what sub shells are included? | 0, 1, 2 s, p, d |
| If the value of n is 4, what is the value of l and what sub shells are included? | 0, 1, 2, 3 s, p, d, f |
| What does the magnetic (ml) value indicate? What are the possible integers? | Indicates the orientation in space of the orbital within a subshell (x-axis, y-axis, z-axis) Possible integer values from -l to +l (including 0) |
| If the sub shell is s, what is the l value and the ml value? | 0 0 |
| If the sub shell is p, what is the l value and the ml value? | 1 -1, 0, 1 |
| If the sub shell is d, what is the l value and the ml value? | 2 -2, -1, 0, 1, 2 |
| If the sub shell is f, what is the l value and the ml value? | 3 -3, -2, -1, 0, 1, 2, 3 |
| What does the spin (ms) indicate, and what are the possible answers? | Indicates the orientation of the spin of the electron Two possibilities: ms= +½ (spin up), ms= -½ (spin down) |
| What is the Pauli Exclusion Principle? | No two electrons in any atoms may have the same set of four quantum numbers No orbital can have more than two electrons, and they must have opposite spins |
| What is electron configuration? | The arrangement of electrons in the orbital |
| Orbitals with the same, have the same ___ value in the same ___ level | n; principal |
| Orbitals with the same values of ___ and ___ are said to be in the same ____ | n and l; sub shell or sub level |
| If the energy level is 4, how many sub levels are there and how many types of sub levels? | 4 s, p, d, f |
| If the energy level is 3, how many sub levels are there and how many types of sub levels? | 3 s, p, d |
| If the energy level is 2, how many sub levels are there and how many types of sub levels? | 2 s, p |
| If the energy level is 1, how many sub levels are there and how many types of sub levels? | 1 s |
| What are the key concepts related to the relative energy of orbitals? | Orbitals in different sub shells have a different energies Orbitals in the same sub shell are degenerate and have the same energy level The lower l value with the same n value means the lower the energy of the corresponding orbitals |
| What are the three principals of filling the orbitals with electrons? | Aufbau principle Pauli exclusion principle Hund's rule |
| Aufbau principle | Electron configurations of the elements is determined by “building” them in order of atomic numbers |
| Pauli exclusion principle | No two electrons in any atom may have the same set of four quantum numbers Each orbital can have a maximum of two electrons, with opposite spins |
| Hund's rule | When filling orbitals that have the same energy, electrons fill singly first then with parallel spins Once the orbitals of equal energy are half full, the electrons start to pair |
| What is short-hand electron configuration? | an abbreviation of the electron configuration that replaces the core electrons with the noble gas symbol in a square bracket |
| Where are the transition elements located? | The d block |
| In transition elements the outermost principal energy is____ | the row number minus one |
| What are the two exceptions to the electron configuration? | Cr and Cu |
| Definition of paramagnetic | Has at least one unpaired electron |
| Definition of diamagnetic | All electrons are paired |
| ____ is attracted to a magnetic field, ___ is repelled by a magnetic field | paramagnetic, diamagnetic |
| What are valence electrons? | the electrons occupying the outermost shell orbital(s), highest value of n |
| Why are valence electrons important? | They are key to chemical properties They are important to bonding |
| Where are the valence electrons in main group elements? | Valence electrons are in the highest s-orbital and p-orbital |
| Where are the valence electrons in transition metals? | valence electrons are two s-electrons plus those in highest incomplete d-orbital |
| What are core electrons? | electrons in complete principle energy levels and those in complete d and f sub levels |
| What is a cation? | positively charged ion that forms when one or more electrons are removed from an atom |
| What is an anion? | negatively charged ion that forms when one or more electrons are added to a parent atom |
| How to obtain the electron configuration of a cation? | Write electron configuration of the neutral atom Subtract the number of electrons indicated by the charge Note: for transition metals the ns electrons are lost first then the electrons in the d orbital |
| How to obtain the electron configuration of an anion? | Write electron configuration of the neutral atom Add the number of electrons indicated by the charge |
| What is Coulomb's law? | Describes the attractions and repulsions between charged particles |
| Following Coulomb's law, how to like charges react with each other, what is the potential energy, and what happens to r as the potential energy decreases? | Like charges repel each other Potential energy is positive Potential energy decreases as r increases |
| Following Coulomb's law, how to opposite charges react with each other, what is the potential energy, and what happens to r as the potential energy decreases? | Opposite charges attract each other Potential energy is negative Potential energy decreases as r decreases |
| What is shielding? | When the electrons closer to the nucleus shield other electrons from experiencing the full positive charge of the nucleus and reduce the attraction to the nucleus when n>= 3 |
| Components and what happens to electrons in an ionic bond | Metal and nonmetal Transferring of electrons |
| Components and what happens to electrons in an covalent bond | Two nonmetals Sharing of electrons |
| Properties of an ionic compound | Strong bonds Have a crystalline structure and be rigid/brittle Have high melting and boiling points Most dissolve readily in water they when dissolve/melt are excellent conductors of electricity and heat Solids are poor conductors of electricity |
| Properties of an covalent compound | Generally have much lower melting and boiling points than ionic compounds Many are liquids or gases at room temperature and insoluble in water In their solid states are typically much softer than ionic solids Poor conductors of electricity in any state |
| What are ionic bonds formed by? | formed by electrostatic forces between cations and anion |
| What are covalent bonds formed by? | formed between two nonmetals when they share valence electrons |
| What is the potential energy of ionic bonds? What is the ionization energy? What is the electron affinity | Metals have relatively low ionization energies, nonmetals have relatively high electron affinities Cations and anions attract each other resulting in lower overall potential energy |
| What is the potential energy of covalent bonds? What is the ionization energy? What is the electron affinity | Nonmetal atoms have high ionization energies and electron affinity the two nonmetals share valence electrons that interact with both nuclei lowering potential energy |
| What is electronegativity? | tendency of an atom to attract bonding electrons to itself in a chemical bond |
| What is the trend of electronegativity? When does it increase | Increases across period to the right and decreases down a column |
| What is a polar covalent bond? | intermediate between a pure covalent bond and an ionic bond that has a positive and negative pole |
| How does a polar covalent bond result in? | Results in unequal sharing of electrons that results in larger electron density in one electron and a smaller electron density than the other |
| If a bond is pure covalent, the bonding electrons are ____, and the electronegativity difference value is ___. | Equally sharing <= 0.4 |
| If a bond is polar covalent, the bonding electrons are ____, and the electronegativity difference value is ___. | Unequally sharing 0.5- 1.8 |
| If a bond is ionic, the bonding electrons are ____, and the electronegativity difference value is ___. | Transferring >= 1.9 |
| What is a lewis structure? | drawing that represents chemical bonds between atoms as shared or transferred electrons |
| What are the steps of drawing a lewis structure? | Write the atomic symbol to represent the nucleus and inner electrons Draw a dot for each valence electron around an atom Put one on each of the four sides, pair them last Maximum of two dots per side |
| What is the octet rule? | tendency of main group atoms to form enough bonds to obtain eight valence electrons in outermost shell to achieve a noble gas configuration |
| What are the exceptions to the octet rule? | Incomplete octet Expanded octet Odd-electron species |
| What is an incomplete octet? | molecules or ions with fewer than eight electrons around an atom |
| What is an Expanded octet? When does it commonly happen? | molecules or ions with more than eight electrons around an atom Common for third or higher period due to accessible d orbitals Never occur when n is less than 3, have to be at least 3 or greater |
| What is an odd-electron species? Are the electrons stable/unstable? Are the electrons reactive/nonreactive? | molecules or ions with an odd number of electrons (called free radicals) They are unstable They are reactive |
| What is a resonance structure? | when two or more valid Lewis structures can be drawn for the same compound |
| What is a resonance hybrid? | average for the resonance forms shown by Lewis structures |
| Do resonance structures exist? Do resonance hybrids exist? | Resonance structures don’t exist, they are simply a way to describe the actual structure, resonance hybrid are the only actual structure that exists |
| What is the bond order of resonance structures? | ratio of the number of chemical bonds around the central atom to the number bond groups around the central atoms |
| What is the bond order equation? | Bond order= number of chemical bonds around the central atoms/ number of bond groups around the central atom |
| What is the delocalization of electrons? | when electrons are not confined to a single bond or atom but are spread out over multiple atoms or bonds |
| What is formal charge? | an electron bookkeeping system that allows us to discriminate between alternative Lewis structures |
| What is the formal charge equation? | Formal charge= # of valence e- - # of nonbonding e- - ½ # bonding e- |
| What are the rules of formal charge? | neutral molecule must add to zero sum of formal charges of all atoms in an ion must equal the ion The closer to zero the better when formal charge cannot be avoided, negative formal charge should be reside on the most electronegative atoms |
| What should you do to achieve the best formal charge if there is a negatively charged bonding atom and a positively charged bonding atom? | If two bonding atoms have opposite formal charges, move electrons from the negatively charged bonding atom to the positively charged bonding atoms to form multiple bonds and neutralize the formal charges |
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