TEAS Chemistry Review

Atoms, Bonds, States of Matter

What subatomic particle defines the specific element?

Protons

Mass Number - Atomic Number gives you what subatomic particle?

Neutrons = M - A

What is an isotope? What do they have a different number of - protons, neutrons, or electrons?

Atoms of the same element that have the same number of protons but a different number of neutrons (and thus a different mass number).

In a neutral atom, the number of protons equals the number of _______.

electrons

Phase change directly from a solid to a gas (Endothermic process, e.g., dry ice).
Phase change directly from a gas to a solid.

Sublimation is solid to gas.

Deposition is gas to a solid. Example: Frost forming on a cold windshield or window on a freezing winter night (water vapor in the air turns straight into ice crystals).

Increasing temperature _________ solubility on solids

increases

Increasing temperature ___________ solubility in gases

decreases

Increasing pressure _________ the solubility of a gas in a liquid

increases (Henry’s Law)

mass number is _______ + ________

protons + neutrons

isotopes are atoms of the same element that vary in number of

neutrons

Describe atomic notation. What number is on top and what’s on the bottom?

Mass number on top (protons + neutrons), atomic number (# of protons)

these have unstable nuclei and can undergo spontaneous nuclear reactions. Can be used to estimate age of materials.

Radioactive isotopes

term for the outermost electron shell of an atom in its uncombined state

valence shell. the valence electrons there determine bonding behavior.

Oxidation-reduction reactions involve the transfer of _________ between reactants

electrons

Combustion reactions involve the reaction of a substance with _________

oxygen

__________ occurs when an ionic compound, like NaCl, dissolves in water and separates into its positive (Na⁺) and negative (Cl⁻) ions. This process allows the solution to conduct electricity, making NaCl an electrolyte.

Dissociation

A _________ speeds up a chemical reaction by lowering the activation energy, allowing reactants to convert into products more efficiently. The ________ itself is not consumed in the reaction.

catalyst

__________ has the highest kinetic energy as the vapor molecules have a high random motion. As a result, they have the maximum amount of kinetic energy.

Gas

A + BC → AC + B would be what type of equation?

single replacement

acids have a low pH and a _____ concentration of H+

high

How many valence electrons do the Alkali Metals and Alkaline Earth Metal groups have?

1 and 2

why are Noble Gases inert?

their outer electron shells are full

which atoms have the smallest radius?

those in the first rows of the periodic table, such as Hydrogen and Helium. Look for some teas chem reviews that go through the table.

in which state of matter are the particles the most organized?

solids - because of the low kinetic energy. in each phase, the particles become more and more disorganized because of increasing kinetic energy. remember gas has the most kinetic energy.

if a question says an acid reacts with a base of the same strength and amount, you’ll have a neutral solution with a pH of

7

In the acid + base formula, the positive ion (cation) always comes from the base. The anion (negative ion) always comes from the ______.

TEAS 7 High-Yield Rule

For the TEAS exam, remember this core formula:

$$\text{Acid} + \text{Base} \rightarrow \text{Salt} + \text{Water}$$

• The cation (positive ion) in the salt always comes from the base.

• The anion (negative ion) in the salt always comes from the acid.

An atom has 11 protons and an atomic mass of 20. How many neutrons does it have? How many electrons?

neutrons = mass - protons, so 9 neutrons.

electrons should equal the protons, so 11.

in a neutralization reaction, the cation of the salt always comes from the

base

What subatomic particles make up a cation of carbon-14?

protons:

neutrons:

electrons:

protons are 6 bc carbon is #6 on the table.

neutrons = mass - protons = 14-6= 8 neutrons.

a neutral carbon atom would have 6 electrons = 6 protons, but since this is a cation, it’s positively charged, meaning it lost 1 electron.

Having 5 electrons gives it a net charge of +1 (6 protons - 5 electrons = +1), satisfying the definition of a cation.

6 protons, 8 neutrons, 5 electrons.

where does electronegativity increase on the periodic table?

upper right

elements located in the same vertical group of the periodic table share the same number of ?

the same number of valence electrons

ionization energy increases where? which group has low ionization energy?

up and to the right, like electronegativity. group 1 has low ionization energy.

How many valence electrons does a neutral atom of Sulfur (Group 16 / VI A) possess?

for main group elements, the group number indicates the valence count. group 16 has 6 valence electrons in their outermost shell.

Which category of elements is generally brittle, poor conductors of heat and electricity, and tends to gain electrons during chemical reactions?

Nonmetals

Name an example of an ionic and covalent bonds

ionic: sodium chloride (NaCl), sulfuric acid

covalent: Hcl, methane (CH4)

ionic bonds are between metals and ________, when electrons are ________ from one atom to another.

metals and nonmetals. in ionic bonds, electrons are transferred.

covalent bonds are between two __________ with similar _____________

nonmetals with similar electronegativities

what is the bond type in H20? What about NaCL?

H2O is covalent, and NaCL is ionic.

What does OIL RIG stand for in oxidation-reduction?

OIL RIG: Oxidation Is Loss of electrons; Reduction Is Gain of electrons.

mass = (equation)

density x volume

a neutralization reaction between an acid and a base produces

salt and water

max number of electrons in each shell

1st: 2, 2nd: 8, 3rd: 18, 4th: 32

what occurs during the formation of an ionic bond?

what about covalent?

ionic: electrons are transferred from one atom to another.

covalent: atoms share a pair of electrons.

the octet rule primarily influences an atom’s

electron configuration

what do elements in the same period all have in common?

number of electron shells (each one top to bottom adds an additional shell)

which states of matter are incompressible?

solids and liquids

term for the temperature at which liquid changes to gas

boiling point