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60 Cards in this Set
- Front
- Back
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Aufbau Principle
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Methods of building electron configuration of atoms/ions by adding one electron at a time as atomic number increases across te rows of the periodic table
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Hund's Rule
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When orbitals of identical energy are available electrons individually occupy those orbitals before pairing up
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Degenerate
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Orbitals of equal energy
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Isoelectronic
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Atoms/Ions that have the same electron configuration/same number of electrons
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Octet Rule
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Atoms tend to gain, lose, and share electrons so that each atom has eight valence Electrons (or 2 for duet rule)
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All electrons have a magnetic spin of...
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1/2 up or 1/2 down
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Elements on the periodic table are organized by...
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Increasing atomic #
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What is more stable? Full or partially full shells?
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Full shells
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Which is more stable? Half full shells or partially full shells?
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Half full shells
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What does atomic size influence?
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Physical and Chemical properties
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Atomic Radii
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The distance between the nuclei of neighboring atoms
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What does the size of an atom depend on?
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How far the outermost electron is from the nucleus and the number of Protons in nucleus
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Trend: The size of an atom generally ___ going down a group
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Increases
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Trend: The size of an atom generally___ going across a period (L-R)
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Decreases
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Trend: As you go across a period, electrons are___ to the same shell # (L-R)
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Added
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Cation
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An Ion that is smaller than the parent atom (has a + charge) , usually a metal
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Anion
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An Ion that is larger than its parent atom (has a - charge) usually a nonmetal
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Ionization Energy
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The amount of energy an atom needs to remove 1 Mole if valence Electrons from 1 Mole of ground state atoms ir ions in the gas phase
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First Ionization Energy (IE1)
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The energy required to remove the highest energy electron from 1 Mole if ground state atoms or ions in the gas phase
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Second/Third Ionization Energy (IE2/IE3 (
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Energy requires to remove a secind/Third electron
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Trend: Successive Ionization Energy always___ in magnitude ex) IE1-IE2
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Increases
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Trend: IE1 generally___ going down a MAIN group
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Decreases
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Trend: IE1 generally___ going across a period (L-R)
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Increases
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Electron Affinity (EA)
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The lilkliness if an atom to gain an electron
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Trend: Electron Affinity generally___ going down a MAIN group
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Increases
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Trend: Electron Affinity generally___ moving across a period depending on electron configuration
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increases or decreases
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Cr+Mo Exception
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Prefer half filled d shell rather than a full s shell Cr-[Ar]4S1 3D5 Mo-[Kr] 5S1 4d5
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Cu+Ag Exception
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Prefer a full d shell and a half filled s shell Cu-[Ar] 4S1 3d10
Ag-[Kr] 5S1 4d10 |
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Electrostatic Potential Energy [Eel] or Coulombic Attraction + equation
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Attraction between opposite charged particles
Eel= C [(Q1 x Q2)/(d)] Eel= 2.31 x 10^-19[(Charge of cation x Charge if anion)/(Distance between neighboring nuclei)] |
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Trend: When Eel is positive = ?
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Unstable
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Trend: When Eel is negative =?
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Stable
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Trend: Electrostatic Potential Energy [Eel] Graph
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Distance at lowest point determines bond length and the energy at the lowest point determines the bond strength
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Naming: Nonmetal-Metal
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1st: Nothing 2nd: "ide"
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Naming: Nonmetal-Nonmetal
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1st: Nothing 2nd: Prefix and "ide" ending
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Naming: Transition Metals
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1st: Cation(Metal)/ Roman Numerals 2nd: "ide" ending
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Electronegativity
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Th ability if an atom in a particular bond to attract electrons to itself
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Trend: Electronegativity generally___ across a period (L-R)
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Increases
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Trend: Electronegativity generally___ as you go up a group except for transition metals
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Increases
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In non polar covalent bonds electrons are____
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Shared equally
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In polar covalent bonds, one atom has a___ electron pull than the other atoms
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stronger
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In Ionic bonds an electron is usually___
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Transfered completely
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Exceptions: Octet Rule
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if you have more or less electrons than can fit
if there are odd numbers of electrons if you Boron and Beryllium |
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Trend: Bond length___ as the number if shared electron pairs increases
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decreases
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Bind Dissociation Enthalpy
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Measurement of bond strength
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Trend: The larger the Bond Dissociation Enthalpy value, the___ the bond
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Stronger
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Formal Charge (FC)
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(Number of valence electrons) - (Number of free electrons) - 1/2 ( number of bond pairs)
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Most favored Lewis Dot Structure is one whose (1. The formal charges of the atoms are equal or closest to___) (2. Any negative formal Charge is found on the most___ atom)
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1. "0" 2. electronegative
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In a chemical reaction, the___ substance is converted into the___ substance
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1. Reactant 2. Product
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Diatomic Elements
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H2, N2, O2, F2, Cl2, Br2, I2
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In a chemical reaction,___ is conserved
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Mass
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In a chemical reaction 🔺(Delta)=?
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Heat was added to the reaction
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Synthesis
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A+B -> AB
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Decomposition
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AB -> A + B
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Replacement
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Ax + B -> A + Bx
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Double Replacement
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Ax + By -> Ay + Bx
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Combustion
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CxHy +O2 -> CO2 + H2O
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Stoichiometry
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The quantitative relationship between the react ants and the products
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% Yield= ?
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[(Actual/Theoretical) x 100] = [(Value found through actual emperimentation/Value found through calculation) x 100]
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Limiting Reactant (LR)
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The substance that depletes before the entire reaction is complete
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How to find the Limiting Reactant (LR)
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Divide given weight by molar weight of said compound /// Which ever us smaller is the Limiting reactant
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