Section 1

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molar mass

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Last updated

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Date created

Mar 1, 2020

Cards (78)

Section 1

(50 cards)

molar mass

Front

To find this, add masses of all elements in a compound together.

Back

least

Front

If pressure is increased to a gaseous reaction at equilibrium, the reaction will shift toward the side with the _________ amount of moles.

Back

compressible

Front

Gases are easily ____________ & expand to fill their container.

Back

unsaturated

Front

A(n) ____________ solution can hold more solute.

Back

increased

Front

Increased temperature = ___________ solubility for solids

Back

pressure

Front

In a gas, this is caused by the force of gas particles colliding with their container walls.

Back

neutrons

Front

neutral charge, found in nucleus

Back

protons

Front

positive charge, found in nucleus

Back

isotope

Front

Same element, different number of neutrons

Back

cross method

Front

This is how you identify the number of ions that will participate in an ionic bond.

Back

mass number

Front

________________ = protons + neutrons

Back

H+

Front

[____] = 1 x 10^-ph

Back

22.4

Front

There are ________ L of gas in 1 mol at STP

Back

equilibrium

Front

At _____________, the rates of the forward and reverse reactions are equal.

Back

ionic

Front

Metal + non-metal = _________ bond

Back

atomic number

Front

Identifies element; number of protons; how the periodic table is organized

Back

electrons

Front

negative charge, around the outside of the nucleus

Back

10

Front

How many electrons will fit in a d subshell?

Back

products

Front

If a reactant is added to a reaction at equilibrium, the reaction will shift toward __________.

Back

strong acid

Front

An acid that completely dissociates in solution

Back

supersaturated

Front

A(n) ____________ solution has more solute than it can hold. This is achieved with heat or stirring.

Back

polar

Front

In a __________ molecule, electrons are not shared evenly (a result of an uneven arrangement of electronegative atoms)

Back

concentration

Front

(M) How much solute vs. solvent there is

Back

net charge

Front

________________ = protons - electrons

Back

4

Front

Total # electrons shared in a double bond

Back

products

Front

If Keq > 1, then _________ are favored.

Back

ionic

Front

What is the strongest bond?

Back

mol/L

Front

M = ?

Back

acid

Front

Sour taste, turns litmus paper red, makes H+ in solutions

Back

reactants

Front

If Keq < 1, then __________ are favored.

Back

base

Front

Taste bitter, slippery, turn litmus paper blue, makes OH- in solutions

Back

mole

Front

6.02 x 10^23 particles of anything

Back

shared

Front

A pair of electrons are ________ for each covalent bond

Back

pH

Front

_____ = -log[H+]

Back

2

Front

How many electrons will fit in an s subshell?

Back

solvent

Front

What does the dissolving

Back

solute

Front

What is dissolved

Back

14

Front

How many electrons will fit in a f subshell?

Back

ion

Front

Same element, different number of electrons

Back

6

Front

How many electrons will fit in a p subshell?

Back

salt

Front

Ionic bonds form this type of compound

Back

decreased

Front

Increased temperature = ___________ solubility for gases

Back

ionic

Front

Which bond has the highest boiling point?

Back

6

Front

Total # electrons shared in a triple bond

Back

8

Front

Most main-group atoms will bond until they have __ electrons in their outer energy level

Back

decimal

Front

Sig Fig rules: Trailing zeros count only if a _______ is present.

Back

covalent

Front

non-metal + non-metal = _________ bond

Back

14

Front

pH + pOH = ?

Back

solute

Front

If the concentration is high, there is a lot of ___________ in a solution.

Back

saturated

Front

A(n) ____________ solution holds as much solute as possible.

Back

Section 2

(28 cards)

alkaline earth metals

Front

Group 2 name

Back

+2

Front

OSN for group 2

Back

halogens

Front

Group 17 name (very electronegative)

Back

reducing agent

Front

The element that is oxidized is also known as the:

Back

oxidation

Front

Loss of electrons is ____________

Back

reduction

Front

Gain of electrons is ____________

Back

oxidizing agent

Front

The element that is reduced is also known as the:

Back

coefficient

Front

When balancing an equation, you can only change this number

Back

basic

Front

pH > 7

Back

endothermic

Front

Products have more energy than the reactants - heat is absorbed

Back

redox

Front

Short for oxidation-reduction

Back

acidic

Front

pH < 7

Back

exothermic

Front

Reactants have more energy than the products - heat is released

Back

-2

Front

OSN for oxygen

Back

decreases

Front

Atomic radius __________ as you move to the right and up on the periodic table

Back

salt, water

Front

Products of acid/base neutralization

Back

reduction

Front

If the oxidation number decreases, this has happened

Back

neutral

Front

pH = 7

Back

increases

Front

Ionization energy __________ as you move to the right and up on the periodic table

Back

temperature

Front

The average kinetic energy of particles in a substance

Back

oxidation

Front

If the oxidation number increases, this has happened

Back

metals

Front

Elements on the left of the periodic table (the majority of elements)

Back

alkali metals

Front

Group 1 name (very reactive)

Back

subscript

Front

When balancing an equation, you cannot change this number

Back

-1

Front

OSN for halogens

Back

non-metals

Front

The elements on the right side of the periodic table

Back

+1

Front

OSN for hydrogen

Back

+1

Front

OSN for group 1

Back