A.L.L.
coyura Academy
THE TEAS 7
CHEMISTRY
CRASH COURSE
Every chemistry concept tested on the ATI TEAS 7 Science section — concise, visual, and exam-ready.
■ ATOMS & ■ CHEMICAL ■ REACTIONS ■ ACIDS, BASES ■ STATES OF
PERIODIC TABLE BONDS & EQUATIONS & SOLUTIONS MATTER
Atomic structure Ionic & covalent Reaction types pH scale & pOH Phases & changes
Isotopes & ions Metallic bonds Balancing equations Acid/base theory Kinetic theory
Periodic trends Polar molecules Conservation of mass Neutralisation Phase diagrams
Element groups IMFs Reaction rates Concentration & molarity PV=nRT gas laws
WHAT TO EXPECT ON THE TEAS 7
Chemistry is part of the Physical Science subcategory (~17% of TEAS Science = ~9 questions).
Topics: atomic structure, periodic table, bonding, reactions, acids/bases, states of matter, and solutions.
Focus on CONCEPTUAL understanding — you will not need a calculator for most questions.
Created by ALLcoyura Academy
, A.L.L.
coyura Academy
ATOMIC STRUCTURE & THE PERIODIC TABLE
The atom is the foundation of all chemistry — know its parts, the periodic table layout, and the trends.
ATOMIC STRUCTURE — THE BUILDING BLOCKS
• Protons: positive charge, located in the NUCLEUS. Number of • Isotopes: same element (same protons), different neutrons.
protons = ATOMIC NUMBER = defines the element. Example: Carbon-12 and Carbon-14 are both carbon.
• Neutrons: no charge, located in the NUCLEUS. Protons + Neutrons • Ions: atom gains electrons → ANION (negative charge). Loses
= ATOMIC MASS (mass number). electrons → CATION (positive charge).
• Electrons: negative charge, orbit the nucleus in ENERGY SHELLS. • Atomic mass on periodic table = weighted average of all
Equal to proton count in neutral atom. naturally occurring isotopes.
• Nucleus: tiny, dense, positively charged core — contains almost all • Valence electrons: electrons in the outermost shell — determine
the mass of the atom. chemical reactivity and bonding.
• Electron shells: K(2), L(8), M(18) — electrons fill from innermost • Noble gases (Group 18) have FULL outer shells → chemically
outward. inert (stable, unreactive).
THE PERIODIC TABLE — LAYOUT & ORGANISATION
Concept Key Facts & TEAS Application
Periods (rows) 7 horizontal rows. As you move ACROSS a period: atomic number increases, electron shells are the same, properties
change dramatically.
Groups (columns) 18 vertical columns. Elements in the SAME GROUP have the same number of valence electrons → similar chemical
properties.
Metals Left and centre of the periodic table (~80% of elements). Shiny, malleable, ductile, good conductors of heat and
electricity.
Non-metals Upper right of the table. Dull, brittle, poor conductors. Includes carbon, nitrogen, oxygen, sulfur, phosphorus,
halogens.
Metalloids Staircase boundary. Silicon, germanium, arsenic — properties intermediate between metals and non-metals. Used in
(semimetals) semiconductors.
Alkali Metals (Group 1) Li, Na, K, Rb, Cs, Fr. ONE valence electron. Highly reactive, soft, form +1 ions. React vigorously with water.
Alkaline Earth Metals Be, Mg, Ca, Sr, Ba, Ra. TWO valence electrons. Less reactive than alkali metals. Form +2 ions.
(Group 2)
Halogens (Group 17) F, Cl, Br, I, At. SEVEN valence electrons. Very reactive non-metals. Form -1 ions. Strong oxidising agents.
Noble Gases (Group He, Ne, Ar, Kr, Xe, Rn. EIGHT valence electrons (He=2). Chemically inert. Used in lighting and as inert atmospheres.
18)
Transition Metals Variable valence electrons. Form coloured compounds, multiple oxidation states. Include Fe, Cu, Zn, Au, Ag.
(Groups 3-12)
PERIODIC TRENDS — PATTERNS ACROSS THE TABLE
Trend Direction & Rule — Left/Right & Up/Down
Atomic Radius DECREASES across a period (L→R) — more protons pull electrons closer. INCREASES down a group — more
electron shells.
Ionisation Energy Energy to remove an electron. INCREASES across a period (harder to remove). DECREASES down a group.
Electronegativity Attraction for electrons in a bond. INCREASES across a period. DECREASES down a group. Fluorine = most
electronegative.
ATOMS & PERIODIC TABLE Created by ALLcoyura Academy Page 2
coyura Academy
THE TEAS 7
CHEMISTRY
CRASH COURSE
Every chemistry concept tested on the ATI TEAS 7 Science section — concise, visual, and exam-ready.
■ ATOMS & ■ CHEMICAL ■ REACTIONS ■ ACIDS, BASES ■ STATES OF
PERIODIC TABLE BONDS & EQUATIONS & SOLUTIONS MATTER
Atomic structure Ionic & covalent Reaction types pH scale & pOH Phases & changes
Isotopes & ions Metallic bonds Balancing equations Acid/base theory Kinetic theory
Periodic trends Polar molecules Conservation of mass Neutralisation Phase diagrams
Element groups IMFs Reaction rates Concentration & molarity PV=nRT gas laws
WHAT TO EXPECT ON THE TEAS 7
Chemistry is part of the Physical Science subcategory (~17% of TEAS Science = ~9 questions).
Topics: atomic structure, periodic table, bonding, reactions, acids/bases, states of matter, and solutions.
Focus on CONCEPTUAL understanding — you will not need a calculator for most questions.
Created by ALLcoyura Academy
, A.L.L.
coyura Academy
ATOMIC STRUCTURE & THE PERIODIC TABLE
The atom is the foundation of all chemistry — know its parts, the periodic table layout, and the trends.
ATOMIC STRUCTURE — THE BUILDING BLOCKS
• Protons: positive charge, located in the NUCLEUS. Number of • Isotopes: same element (same protons), different neutrons.
protons = ATOMIC NUMBER = defines the element. Example: Carbon-12 and Carbon-14 are both carbon.
• Neutrons: no charge, located in the NUCLEUS. Protons + Neutrons • Ions: atom gains electrons → ANION (negative charge). Loses
= ATOMIC MASS (mass number). electrons → CATION (positive charge).
• Electrons: negative charge, orbit the nucleus in ENERGY SHELLS. • Atomic mass on periodic table = weighted average of all
Equal to proton count in neutral atom. naturally occurring isotopes.
• Nucleus: tiny, dense, positively charged core — contains almost all • Valence electrons: electrons in the outermost shell — determine
the mass of the atom. chemical reactivity and bonding.
• Electron shells: K(2), L(8), M(18) — electrons fill from innermost • Noble gases (Group 18) have FULL outer shells → chemically
outward. inert (stable, unreactive).
THE PERIODIC TABLE — LAYOUT & ORGANISATION
Concept Key Facts & TEAS Application
Periods (rows) 7 horizontal rows. As you move ACROSS a period: atomic number increases, electron shells are the same, properties
change dramatically.
Groups (columns) 18 vertical columns. Elements in the SAME GROUP have the same number of valence electrons → similar chemical
properties.
Metals Left and centre of the periodic table (~80% of elements). Shiny, malleable, ductile, good conductors of heat and
electricity.
Non-metals Upper right of the table. Dull, brittle, poor conductors. Includes carbon, nitrogen, oxygen, sulfur, phosphorus,
halogens.
Metalloids Staircase boundary. Silicon, germanium, arsenic — properties intermediate between metals and non-metals. Used in
(semimetals) semiconductors.
Alkali Metals (Group 1) Li, Na, K, Rb, Cs, Fr. ONE valence electron. Highly reactive, soft, form +1 ions. React vigorously with water.
Alkaline Earth Metals Be, Mg, Ca, Sr, Ba, Ra. TWO valence electrons. Less reactive than alkali metals. Form +2 ions.
(Group 2)
Halogens (Group 17) F, Cl, Br, I, At. SEVEN valence electrons. Very reactive non-metals. Form -1 ions. Strong oxidising agents.
Noble Gases (Group He, Ne, Ar, Kr, Xe, Rn. EIGHT valence electrons (He=2). Chemically inert. Used in lighting and as inert atmospheres.
18)
Transition Metals Variable valence electrons. Form coloured compounds, multiple oxidation states. Include Fe, Cu, Zn, Au, Ag.
(Groups 3-12)
PERIODIC TRENDS — PATTERNS ACROSS THE TABLE
Trend Direction & Rule — Left/Right & Up/Down
Atomic Radius DECREASES across a period (L→R) — more protons pull electrons closer. INCREASES down a group — more
electron shells.
Ionisation Energy Energy to remove an electron. INCREASES across a period (harder to remove). DECREASES down a group.
Electronegativity Attraction for electrons in a bond. INCREASES across a period. DECREASES down a group. Fluorine = most
electronegative.
ATOMS & PERIODIC TABLE Created by ALLcoyura Academy Page 2
