Chemistry Terms
Electron Configurations
Formulas, Equations, and Constants
Balancing Equations
Random Chem Knowledge
100
Reaction in which energy is released from the system, making the surroundings warmer

Exothermic Reaction

100

Define electron configuration.

The representation of the arrangement of electrons distributed among the orbital shells and subshells.

100

What is the Ideal Gas Law?

PV = nRT

100

Balance the following equations:

C3H8 + O2 --> CO2 +  H2O

C3H8 + 5O2 --> 3CO2 + 4H2O

100
State Faraday's Constant and the units it's given in

F = 96,500 coulomb's per mole of electrons

200

Usually reversible change to a substance's properties such as size, shape, or state of matter.

Physical Change

200

What is the maximum number of electrons each subshell can contain? (SPDF)

S=2, P=8, D=18, F=32

200

What is Avogadro's number?

6.022 * 10-23 J/K

200

Balance the following equation: 

Be2C + H2O --> Be(OH)2 + CH4

Be2C + 4H2O --> 2Be(OH)2 +CH4

200

Which of the following has the biggest 1st ionization energy?

Na, Mg, Al, Si

Silicon (Si)

300

Assumes that each atom in a molecule will achieve a geometry that minimizes the repulsion between electrons in the valence shell of that atom.

VESPR Theory

300

Name of of the three important rules of electron configuration.

Aufbau Principle, Pauli-Exclusion Principle, and Hund's Rule

300

What is the equation to solve for pH when the solution is buffering?

pH = pKa + log[A-]/[HA]


300

Balance the following equation:

Al2(SO3)3 + NaOH --> NaSO3 + Al(OH)3

Al2(SO3)3 + 6NaOH --> 3Na2SO3 + 2Al(OH)3

300

What do you call the attractive force resulting when polar molecules line up so that the positive and negative ends are close to each other?

A dipole-dipole attraction

400

A measure of the energy released or consumed when one mole of a substance is created under standard conditions from its pure elements.

Standard Enthalpy of Formation

400

Electrons must occupy empty orbitals in the same sublevel singly before they pair up in the same orbital.

Hund's Rule

400

What is the equation for calculating change in G at standard conditions using the given temperature and equilibrium constant, K?

Delta G = RTlnK ("Rat Link" equation)

400

Balance the following equation:

S + HNO3 --> H2SO4 + NO2 + H2O

S + 6HNO3 --> H2SO4 + 6NO2 + 2H2O

400

Name all 7 common strong acids

(Bonus 200 points if you can name them all in order of strongest to weakest pH)

Perchloric acid (HClO4), Hydroiodic acid (HI), Hydrobromic acid (HBr), Hydrochloric acid (HCl), Sufuric acid (H2SO4), Nitric acid (HNO3), Chloric acid (HClO3)

500

A species that has the potential to act both as an acid and as a base according to Brønsted-Lowry Theory.

Amphoteric Compound

500

[WITHOUT LOOKING AT A PERIODIC TABLE]

What is the electron configuration of sodium?

1s22s22p63s1

500

What is the gas constant value you should use when utilizing the Ideal Gas Law equation?

R = 0.0821 L*ATM/mol*K

500

Balance the following equation:

Cu + HNO3 --> Cu(NO3)2 + NO + H2O

3Cu + 8HNO3 --> 3Cu(NO3)2 + 2NO + 4H2O

500

Which of the following species is NOT planar?

A.) CO32-

B.) NO3-

C.) BF3

D.)PCl 3

D.) PCl3

The electron pair causes a disruption in the planar compound. Each individual chlorine atom experiences repulsion from the lone electron pair,  causing the Cl atoms to bend together. This gives this compound a trigonal pyramidal shape instead of a planar geometry.

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