1. Basic Atomic Structure

🧪 Table: Parts of an Atom

Component	Description
Protons	A stable subatomic particle in the atomic nuclei with a positive charge equal in magnitude to that of an electron, but of opposite sign.
Neutrons	A subatomic particle of about the same mass as a proton but without an electrical charge.
Electrons	A negatively charged subatomic particle that is 1/1836 times smaller than a proton.
Electric Charge	- Neutrons = Neutral - Protons = Positive - Electrons = Negative
Important Note	The number of protons and electrons is equal in a neutral atom.

❓ Flashcard Questions (Numbered)

1. What subatomic particle has a positive charge and is found in the atomic nucleus?

2. Which subatomic particle has nearly the same mass as a proton but no charge?

3. Which subatomic particle is much smaller than a proton and carries a negative charge?

4. What does it mean when a neutron is called "neutral"?

5. How much smaller is an electron compared to a proton?

6. What is the relationship between protons and electrons in a neutral atom?

7. Which particle has a charge equal in magnitude to an electron but opposite in sign?

8. What can you infer about the charge of an atom if it has more electrons than protons?

• Proton

• Neutron

• Electron

• It has no electrical charge

• 1/1836 times smaller

• They are equal in number

• Proton

• The atom would have a negative charge

Explain what each number mean in this screenshot

Component	Mass	Mass Unit	Notes
Proton	1.67 × 10⁻²⁴ g	1 amu	Found using atomic number
Neutron	1.67 × 10⁻²⁴ g	1 amu	Mass similar to proton
Electron	9.109 × 10⁻²⁸ g	0.000549 amu	Not counted in atomic mass
Atomic Number	Number of protons in an element	—	Also equals number of electrons in a neutral atom
Atomic Mass	Number of protons + neutrons in an element	—	Used to calculate neutron number
Neutron Formula	Neutrons = Mass Number − Atomic Number	—	Example: Oxygen has 8 protons and 8 neutrons
Mnemonic: PAN MAN	- P = Protons - A = Atomic Number - N = Number of Protons - M = Mass Number - A = Add - N = Neutrons	—	Helps memorize relationships between protons, mass, and neutrons

What does amu stands for?

AMU stands for atomic mass unit.

What is Isotopes

Distinct, Nuclear species of the same chemical element.

They have the same atomic number and position in the periodic table.

They have the same number of protons but different numbers of neutrons.

❓ TEAS-Style Multiple Choice Questions (Isotopes & Atomic Structure)

1. Which of the following best defines an isotope?
   A. Atoms with different numbers of protons and electrons
   B. Atoms with the same number of protons but different numbers of neutrons
   C. Atoms with different numbers of protons and neutrons
   D. Atoms with the same mass number but different atomic numbers

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2. If two atoms are isotopes of the same element, what must be true?
   A. They have the same number of neutrons
   B. They have the same number of protons
   C. They have different atomic numbers
   D. They have different numbers of electrons

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3. Which subatomic particle determines the identity of an element?
   A. Neutron
   B. Electron
   C. Proton
   D. Mass number

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4. What is the mass number of an atom with 11 protons and 12 neutrons?
   A. 12
   B. 11
   C. 23
   D. 1

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5. Why do isotopes of an element have nearly identical chemical behavior?
   A. They have the same number of neutrons
   B. They have the same atomic mass
   C. They have the same number of electrons
   D. They have the same number of nucleons

✅ Answer Table (Correct Answers Only)

Question	Correct Answer	Choice Text
1	B	Atoms with the same number of protons but different numbers of neutrons
2	B	They have the same number of protons
3	C	Proton
4	C	23
5	C	They have the same number of electrons

❓ TEAS-Style Multiple Choice Questions (Ions and Cations)

1. What is an ion?
   A. An atom with no charge
   B. An atom or group of atoms with a net electrical charge
   C. An atom with an equal number of protons and electrons
   D. An atom that always has a positive charge

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2. How does an atom become a cation?
   A. By gaining electrons
   B. By losing protons
   C. By losing electrons
   D. By gaining neutrons

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3. Which of the following describes a cation?
   A. A negatively charged ion
   B. A neutral atom
   C. A positively charged ion
   D. An atom with more electrons than protons

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4. What charge does a sodium cation (Na⁺) have?
   A. -1
   B. +1
   C. 0
   D. +2

CATION VS ANION

Term	Definition
Ion	An atom or a group of atoms with a net electrical charge. An atom becomes an ion if it gains or loses electrons.
Cation	A positively charged ion. Formed when an atom loses electrons.

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Example: Sodium (Na)

State	Protons (+)	Electrons (−)	Charge
Neutral Sodium (Na)	11	11	No charge (neutral)
Sodium Cation (Na⁺)	11	10	+1 charge (cation)

• Sodium atom loses 1 electron → becomes Na⁺ (cation).

• Protons stay the same (11), electrons decrease to 10, resulting in a net +1 charge.

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Memory Tip:

"Cats have PAWS"

• Cation is a "PAW"itive ion.

• Helps remember that cations are positive ions.

✅ Answer Table (Correct Answers Only)

Question	Correct Answer	Choice Text
1	B	An atom or group of atoms with a net electrical charge
2	C	By losing electrons
3	C	A positively charged ion
4	B	+1

❓ TEAS-Style Multiple Choice Questions (Anions and Ions)

1. What is an ion?
   A. An atom with no charge
   B. An atom or group of atoms with a net electrical charge
   C. An atom with equal numbers of protons and electrons
   D. An atom that always has a positive charge

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2. How does an atom become an anion?
   A. By gaining electrons
   B. By losing protons
   C. By losing electrons
   D. By gaining neutrons

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3. Which of the following describes an anion?
   A. A positively charged ion
   B. A neutral atom
   C. A negatively charged ion
   D. An atom with more protons than electrons

CATION VS ANION

Term	Definition
Ion	An atom or group of atoms with a net electrical charge. An atom becomes an ion if it gains or loses electrons.

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ANION

Example: Oxygen (O)	Before Gaining Electrons	After Gaining Electrons
Protons (+)	8	8
Electrons (-)	8 (neutral, no charge)	10 (gained 2 electrons)
Charge	Neutral (no charge)	Negative ion, charge = 2- (O²⁻)

• Anion is a negatively charged ion formed when an atom gains electrons.

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Memory Tip:

"An anion is a negative ‘onION’."

• Helps remember that anions have negative charges.

✅ Answer Table (Correct Answers Only)

Question	Correct Answer	Choice Text
1	B	An atom or group of atoms with a net electrical charge
2	A	By gaining electrons
3	C	A negatively charged ion

🧪 What is a Nucleus in Chemistry?

Property
Location ?
Charge ?
Mass ?
Size ?
Held together by ?

In chemistry, the nucleus is the central core of an atom. It contains:

• Protons (positively charged particles)

• Neutrons (neutral particles with no charge)

🔑 Key Facts About the Nucleus:

Property	Details
Location	Center of the atom
Charge	Positive (because of the protons)
Mass	Contains nearly all of the atom's mass
Size	Extremely small compared to the entire atom
Held together by	Strong nuclear force (overcomes repulsion between positive protons)

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🧠 Quick Analogy:

If an atom were the size of a football stadium, the nucleus would be like a tiny marble at the center—but it holds almost all the atom’s mass!

Revisit Shells, Subshells and Orbits Part 1

❓ Flashcard Questions

1. What subshell is available in the K shell (n=1)?

2. Which shell has the subshells s and p?

3. At which energy level does the d subshell first appear?

4. What is the shell name for n=4?

5. Which subshells are available in the N shell?

6. Which subshells are common to both the M and N shells?

7. What shell includes only the s subshell?

8. What is the shell name that contains s, p, and d subshells but not f?

9. Which energy level introduces the f subshell?

10. How do shells relate to energy levels in an atom?

11. Which electrons are involved in chemical bonding according to the diagram?

12. What is a subshell?

n (Energy Level)	Shell Name	Available Subshells
n = 1	K shell	s
n = 2	L shell	s, p
n = 3	M shell	s, p, d
n = 4	N shell	s, p, d, f

Note: Only Electrons in the outermost shell participate in chemical bonds.

✅ Flashcard Answers

1. The s subshell.

2. The L shell (n=2).

3. At n=3, the M shell.

4. N shell.

5. s, p, d, and f.

6. s, p, and d.

7. K shell (n=1).

8. M shell (n=3).

9. Energy level n=4.

10. Shells are energy levels where electrons orbit the nucleus.

11. Only electrons in the outermost shell participate in chemical bonds.

12. A subshell is a subdivision of electron shells separated by electron orbitals.

Revisit Shells, Subshells and Orbits Part 2

What is the subshell shape of each Shell Number

❓ Flashcard Questions

1. How many orbitals are in the s subshell?

2. What is the maximum number of electrons in shell number 1?

3. Which subshells are present in shell number 2?

4. What is the total number of orbitals in shell 3?

5. How many electrons can shell 3 hold in total?

6. What are the subshells and orbital counts in shell number 4?

7. Which subshell can hold up to 14 electrons?

8. How many electrons can fit into the p subshell of any shell?

9. What is the electron configuration of magnesium (atomic number 12)?

10. In which shell is the 3d orbital found?

11. How many electrons can fit in the 4f subshell?

12. What is the total electron capacity of shell number 4?

📊 Table: Orbital Structure by Shell Number

Shell Number	Subshell Designation	Number of Orbitals	Number of Electrons	Subshell Designation
1	s	1	2
2	s, p	1, 3	8 (2s = 2, 2p = 6)
3	s, p, d	1, 3, 5	18 (3s = 2, 3p = 6, 3d = 10)
4	s, p, d, f	1, 3, 5, 7	32 (4s = 2, 4p = 6, 4d = 10, 4f = 14)

ATI Quiz point:

They love asking the

• characteristic of the d shell/orbital: Circular Sphere

• characteristic of the p shell/orbital: Dumbbell

• characteristic of the d shell/orbital: Four Leaves Clover

• characteristic of the f shell/orbital: Come in different Shapes

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⚛ Bonus Detail:

• Magnesium (Atomic Number 12) Electron Configuration:
  1s² 2s² 2p⁶ 3s²

✅ Flashcard Answers

1. 1 orbital.

2. 2 electrons.

3. s and p subshells.

4. 9 orbitals (1 from s, 3 from p, 5 from d).

5. 18 electrons.

6. Subshells: s, p, d, f. Orbitals: 1, 3, 5, 7.

7. The f subshell.

8. 6 electrons.

9. 1s² 2s² 2p⁶ 3s².

10. In shell number 3.

11. 14 electrons.

12. 32 electrons.

How a chemical become stable?

Ionic Bonds

Ionic Bone: Complete transfer of valence electron(s) between Atoms

🧪 What's Happening in the Diagram?

Sodium (Na)	Chlorine (Cl)
Atomic # = 11	Atomic # = 17
Electron config: 2, 8, 1 → 1 valence e⁻	Electron config: 2, 8, 7 → 7 valence e⁻
Not stable	Not stable
Loses 1 electron to become Na⁺ (stable with 8 in second shell)	Gains 1 electron to become Cl⁻ (stable with 8 in third shell)

⚛ Type of Bond: Ionic Bond

• Definition: A complete transfer of electrons from one atom to another.

• Sodium gives an electron.

• Chlorine takes that electron.

• Now, both have full outer shells.

• The result is Na⁺ and Cl⁻, which are oppositely charged and attract.

• This forms NaCl (table salt).

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📏 Octet Rule Reminder:

Atoms are most stable when they have 8 electrons in their outer shell (except for the first shell, which is full at 2).

They might lose, gain or share electrons

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🧠 Memory Tip from the Slide:

"I take, you give" → Describes the electron transfer in an ionic bond.

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✅ Summary: How Ionic Bonding Leads to Stability

1. Sodium has 1 electron in its outer shell → gives it away → becomes stable.

2. Chlorine needs 1 electron to complete its outer shell → takes one → becomes stable.

3. This transfer creates charged ions (Na⁺ and Cl⁻) that are held together by electrostatic attraction.

Ionic Bonds Quiz:

🧪 TEAS-Style Practice Questions

#	Question
1	Which of the following is true of sodium (Na) in an ionic bond with chlorine (Cl)? A. It gains one electron B. It shares one electron C. It loses one electron D. It becomes negatively charged
2	What is the total number of valence electrons in chlorine before bonding with sodium? A. 6 B. 7 C. 8 D. 1
3	What type of bond forms between sodium and chlorine in NaCl? A. Covalent B. Metallic C. Hydrogen D. Ionic
4	Why does sodium form an Na⁺ ion during bonding? A. To gain a full outer shell of 10 electrons B. To lose an electron and achieve a stable electron configuration C. To match chlorine’s mass number D. Because sodium has more neutrons than electrons
5	What is the charge on a chlorine ion (Cl⁻) after it gains an electron from sodium? A. 0 B. +1 C. -1 D. -2
6	What rule explains why atoms form chemical bonds to get 8 electrons in their outer shell? A. Isotope rule B. Periodic rule C. Bonding principle D. Octet rule
7	In an ionic bond, electrons are: A. Shared equally B. Shared unequally C. Completely transferred D. Ignored
8	After forming NaCl, how many electrons are in sodium’s outermost shell? A. 1 B. 8 C. 0 D. 2

✅ Answer Key

#	Correct Answer
1	C. It loses one electron
2	B. 7
3	D. Ionic
4	B. To lose an electron and achieve a stable electron configuration
5	C. -1
6	D. Octet rule
7	C. Completely transferred
8	B. 8

Covalent Bond

📘 TEAS-Style Questions (Covalent Bonds) Question 1:

Which of the following best describes a covalent bond?

A. Transfer of electrons from one atom to another
B. Sharing of protons between atoms
C. Sharing of electrons between atoms
D. Attraction between ions of opposite charges

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Question 2:

What is the total number of electrons in a carbon atom?

A. 4
B. 6
C. 8
D. 12

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Question 3:

What do oxygen atoms need in order to achieve a full outer shell?

A. 1 more proton
B. 2 more electrons
C. 4 more neutrons
D. To lose 2 electrons

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Question 4:

Which of the following elements mostly forms covalent bonds?

A. Sodium
B. Magnesium
C. Chlorine
D. Hydrogen

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Question 5:

How many electrons does carbon need to complete its outer shell?

A. 2
B. 4
C. 6
D. 8

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Question 6:

What is the memory trick associated with covalent bonding?

A. Give to grow
B. Sharing is caring
C. Gain to maintain
D. Attract to react

Category	Details
Bond Type	Covalent Bond
Description	Sharing of electrons to form electron pairs between atoms
Memory Trick	Sharing is caring
Carbon Atom	Protons (+): 6 Neutrons (⌀): 6 Electrons (-): 6
Oxygen Atom	Protons (+): 8 Neutrons (⌀): 8 Electrons (-): 8
Electron Needs (Carbon)	Needs 4 electrons in the outer shell
Electron Needs (Oxygen)	Needs 2 more electrons in outer shell
4 Major Elements Mostly form covalent bonds	Carbon, Oxygen, Hydrogen, Nitrogen
Bond Type of Major Elements	Mostly form covalent bonds

✅ Answer Key

Question	Correct Answer	Explanation
1	C. Sharing of electrons between atoms	This is the defining trait of covalent bonding.
2	B. 6	A carbon atom has 6 protons, 6 neutrons, and 6 electrons.
3	B. 2 more electrons	Oxygen needs 2 electrons to complete its outer shell.
4	D. Hydrogen	Hydrogen, along with carbon, oxygen, and nitrogen, primarily forms covalent bonds.
5	B. 4	Carbon needs 4 electrons to fill its valence shell.
6	B. Sharing is caring	This phrase helps remember the concept of electron sharing in covalent bonds.

Periodic Table

For the test, we need to know what is Period & Group

🧪 What is a Period in the Periodic Table?

• A period is a horizontal row in the periodic table.

• There are 7 periods in total, numbered from 1 to 7.

• As you move from left to right across a period:

  • The atomic number increases.

  • Elements become less metallic and more non-metallic.

  • Electrons are added to the same outer shell.

The period number of an element tells you how many electron shells (energy levels) the atom has.

✅ Example:
Carbon (C), Nitrogen (N), and Oxygen (O) are all in Period 2 – they each have electrons filling their second energy level (shell).

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🧲 What is a Group in the Periodic Table?

• A group is a vertical column in the periodic table.

• There are 18 groups, numbered from 1 to 18.

• Elements in the same group:

  • Have the same number of electrons in their outer shell (valence electrons).

  • Tend to have similar chemical properties.

✅ Example:

• Group 1 = Alkali metals (e.g., Lithium, Sodium) – all have 1 valence electron and are very reactive.

• Group 17 = Halogens (e.g., Fluorine, Chlorine) – all have 7 valence electrons and are also very reactive.

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🔁 Quick Comparison

Feature	Period	Group
Direction	Horizontal row	Vertical column
Total Number	7	18
Key Pattern	Increasing energy levels	Similar valence electron patterns
Example	C, N, O in Period 2	F, Cl, Br in Group 17 (Halogens)