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64 Cards in this Set
- Front
- Back
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Who invented the metal foil experiment? |
Ernest Rutherford. |
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What did the metal foil experiment consist of? |
An alpha source, a thin metal foil, and a photographic screen. He expected all the particles to go through but 2% deflected or bounced back |
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What letter represents the atomic number? |
Z |
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What is a WAVE? |
A progressive, repeating disturbance that spreads through a medium (sound) |
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Electromagnetic Wave |
Originates from the movement of electric charges. Doesn’t require any medium! |
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What does amplitude indicate? |
Intensity |
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Electromagnetic Spectrum |
Complete range of wavelength and frequencies. Another names include EMR (electromagnetic radiation) and Continuous Spectrum. |
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Emission Spectrum |
A record of emitted light |
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Who said “certain atoms in a heated solid can only absorb or emit EMR in a certain, discrete amount”? |
Max Planck |
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What is a Quantum? |
The smallest unit of energy. Magnitude of a quantum is h*frequency. h=6.626x10^-34 (Planck’s Constant) |
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What is a Photon? |
Little packets of EMR, energy treated as a particle. Energy of a photon is E=h*frequency(v) |
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What is Rutherford’s Nuclear Theory? |
1. Electrons can not be stationary 2. Electrons are in motion to overcome attraction to the nucleus 3. Electrons give off a continuous emission of light
4. Electrons are unstable |
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Who said “electrons can only be specified values (quantized)”? |
Niels Bohr |
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How do you calculate electron energy (En)? |
En= -B/n^2 B=2.179x10^-18 (bohrs constant) N= energy level |
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What does a negative electron energy (En) indicate? |
It indicates a force of attraction to the nucleus |
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What is the Ground State for electrons? |
Their normal location |
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What is the Excited State of electrons? |
The location of electrons when energy is absorbed |
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What is the formula for the excited state? |
B(1/ni^2-1/nf^2) N=energy level B=bohrs constant |
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Final energy level > initial energy level |
Absorbed energy |
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What are the 3 problems of Bohr’s theory? |
1. Based on Hydrogen 2. 2D 3. Electrons are much harder to locate in reality |
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What is Wave-Particle Duality of Light? |
Light can be described as a particle and a wave |
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Who said “matter can behave as a wave?” |
Louis de Broglie Wavelength = plancks constant*frequency |
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What is Quantum Mechanics? |
The Who diTheory of atomic structure that treats electrons as wave |
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Who discovered Quantum Mechanics? |
Erwin Schrodinger |
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The Wave Function serves to solve the Wave Equation. To find the probability of finding an electron in a particular volume of space you use the formula- |
Wave Function^2 |
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How many energy level shells are there? |
7 |
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How many energy level sub shells are there? |
S, p, d, f. We count them as 0,1,2,3 |
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Electron configuration shows- |
Subshells |
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Orbital diagrams show |
Orbitals in the form of arrows |
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What is the Aufbau Principle? |
To build an atom, one electron at a time. A rule that electrons always occupy orbitals of the lowest energy possiblewhat |
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Anions |
Add electrons to the valence shell (negative) |
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Cations |
Lose electrons from the valence shell (positive) |
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How does Magnetism work? |
A single electron creates a magnetic field. Paired electrons balance each other out. |
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Diamagnetism |
Repels an external magnetic field |
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Paramagnetic |
Strongly attracted to an external field |
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Which has a larger atomic radius? Cations or anions? |
Anions get lrger Cations get smaller |
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What are Isoelectric Particles? |
Particles with same # of electrons |
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What is Ionization Energy? |
The amount of energy it takes to remove an electron from a ground state atom |
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What is Electron Affinity? |
The amount of energy given off when an electron is added to an atom. Always negative value. |
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What part of the periodic table has the highest IE and EA levels? |
Top right hand corner |
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Ionization energies are usually _________ while electron affinity values are usually ____________. (Positive/Negative) |
IE = positive values EA= negative values |
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Metals tend to lose/gain electrons to form cations/anions |
Metals tend to lose electrons and form cations |
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Nonmetals tend to gain/lose electrons to form cations/anionsu |
Nonmetals tend to gain electrons to form anions. |
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Why do noble gases have a high EA and IE? |
They have no desire to gain or lose electrons. |
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How do Ionic Bonds Occur? |
Through electron transfer (metal and nonmetal) |
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How do covalent bonds occur? |
Electron sharing |
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What is the change in enthalpy? |
The change in heat of a chemical reaction at a constant pressure |
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A negative enthalpy is a______ reaction |
Exothermic |
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A positive enthalpy is a _____ |
Endothermic reaction |
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Born-Haber Cycle Steps |
1. Substances start in room temp 2. Convert to gas 3. Form ions 4. Use IE, EA, and lattice energy |
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What is Lattice energy? |
Energy given off when 1 mol of compound forms gaseous ions. Energy stored in crystal lattice. |
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Nonpolar covalent bond |
Bonding pair is shared equally |
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Polar covalent bond |
Bonding pair is not shared equally |
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What is Electronegativity? |
The ability of an atom to attract electrons to itself when in a molecule |
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What is Coordinate Covalent Bond? |
When one atom provides both electrons of the shared pair |
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These |
Oxygen |
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These two gases are never at the center of a Lewis dot structure |
Oxygen or Hydrogen |
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THESE TWO ELEMENTS CREATE INCOMPLETE OCTETS |
Be - 4 Val e (2 bonds) B - 6 val e (3 bonds) |
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THESE TWO ELEMENTS CREATE EXPANDED OCTETS |
P - 10 Val e (5 bonds) S - 12 Val e (6 bonds) +Halogens |
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How does bond order (amount of lines between 2 Lewis dot element things) affect bond length? |
Bond order up=bond length down |
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How do polar covalent bonds affect bond length? |
The bond length is shorter than expected |
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**** you cram |
Dick face |
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**** |
Cutn |
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I hate you |
You ******* hag |
