What type of bond involves the sharing of electrons?

Covalent bond. Covalent bonds involve the sharing of electrons between atoms (usually nonmetals). Ionic bonds involve the transfer of electrons from one atom to another.

A substance with a pH of 3 would be classified as:

An acid. pH below 7 indicates an acid. pH 3 is moderately acidic. The lower the pH, the more acidic the substance. Examples at pH 3 include orange juice and vinegar.

In the equation 2H₂ + O₂ → 2H₂O, what type of reaction is this?

Synthesis. This is a synthesis reaction where two or more reactants combine to form a single product. Hydrogen and oxygen combine to form water. The pattern is A + B → AB.

4.8 Chemistry Basics | ATI TEAS 7 (Nursing Admission) | Free Exam Prep

Chemistry Basics

The TEAS tests fundamental chemistry concepts including atomic structure, chemical bonding, reactions, and solutions. These concepts apply to understanding medications, body chemistry, and laboratory values.

Atomic Structure

Component	Charge	Location	Mass
Proton	Positive (+)	Nucleus	1 amu
Neutron	Neutral (0)	Nucleus	1 amu
Electron	Negative (-)	Electron shells	~0 amu

Key numbers:

Atomic number = number of protons (defines element)
Mass number = protons + neutrons
Atomic mass = weighted average of isotopes

The Periodic Table

Group	Elements	Properties
Alkali metals	Li, Na, K	Highly reactive, 1 valence electron
Alkaline earth metals	Mg, Ca	Reactive, 2 valence electrons
Halogens	F, Cl, Br, I	Very reactive nonmetals, 7 valence electrons
Noble gases	He, Ne, Ar	Unreactive, full outer shell (8 electrons)

Periods: Horizontal rows (indicate electron shells) Groups: Vertical columns (similar properties)

Chemical Bonding

Bond Type	Description	Example
Ionic	Transfer of electrons	NaCl (table salt)
Covalent	Sharing of electrons	H₂O (water)
Hydrogen	Weak attraction between H and O/N/F	Water molecules

Ionic bonds: Form between metals and nonmetals Covalent bonds: Form between nonmetals

Types of Chemical Reactions

Type	Description	Example
Synthesis	A + B → AB	2H₂ + O₂ → 2H₂O
Decomposition	AB → A + B	2H₂O → 2H₂ + O₂
Single replacement	A + BC → AC + B	Zn + 2HCl → ZnCl₂ + H₂
Double replacement	AB + CD → AD + CB	AgNO₃ + NaCl → AgCl + NaNO₃
Combustion	Fuel + O₂ → CO₂ + H₂O	CH₄ + 2O₂ → CO₂ + 2H₂O

Balancing Chemical Equations

Law of Conservation of Mass: Atoms are neither created nor destroyed.

Steps:

Count atoms on each side
Add coefficients to balance
Check your work

Example: Balance H₂ + O₂ → H₂O

Unbalanced: 2 H, 2 O → 2 H, 1 O
Balanced: 2H₂ + O₂ → 2H₂O

Acids and Bases

Property	Acids	Bases
pH	Below 7	Above 7
H⁺ ions	Donate H⁺	Accept H⁺
Taste	Sour	Bitter
Feel	—	Slippery
Examples	HCl, vinegar, citrus	NaOH, ammonia, soap

pH Scale

pH	Classification	Examples
0-2	Strong acid	Stomach acid (pH 1-2)
3-6	Weak acid	Coffee (pH 5), urine (pH 6)
7	Neutral	Pure water
8-11	Weak base	Blood (pH 7.4), baking soda
12-14	Strong base	Bleach (pH 13)

Solutions

Term	Definition
Solute	Substance being dissolved (smaller amount)
Solvent	Substance doing the dissolving (larger amount)
Solution	Homogeneous mixture of solute and solvent
Concentration	Amount of solute per unit of solution

Types of solutions:

Saturated: Maximum solute dissolved
Unsaturated: Can dissolve more solute
Supersaturated: More solute than normally possible

Factors Affecting Solubility

Factor	Effect on Solubility (solid in liquid)
Temperature	Usually increases solubility
Pressure	Little effect on solids
Stirring	Speeds dissolving (not amount)
Particle size	Smaller particles dissolve faster

Energy in Reactions

Type	Energy	Temperature
Exothermic	Releases energy	Feels warm
Endothermic	Absorbs energy	Feels cold

Healthcare Chemistry Applications

Application	Chemistry Concept
Blood pH regulation	Acid-base balance
Medication concentration	Solutions
IV fluids	Osmolarity
Drug interactions	Chemical reactions

ATI TEAS 7

1Introduction to the ATI TEAS

2Reading

3Mathematics

4Science

5English and Language Usage

Key Takeaways