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Questions and Answers
Who is known as the Father of the Periodic Table?
Who is known as the Father of the Periodic Table?
Which scientist proposed the 'Law of Octaves'?
Which scientist proposed the 'Law of Octaves'?
What was the significant contribution of Henry Moseley to the periodic table?
What was the significant contribution of Henry Moseley to the periodic table?
What was the method used by Johann Wolfgang Döbereiner to classify elements?
What was the method used by Johann Wolfgang Döbereiner to classify elements?
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What was a limitation noted in John A. Newlands' 'Law of Octaves'?
What was a limitation noted in John A. Newlands' 'Law of Octaves'?
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What distinguishes a molecule from a compound?
What distinguishes a molecule from a compound?
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Which statement best describes an ion?
Which statement best describes an ion?
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How many protons are present in an atom of oxygen?
How many protons are present in an atom of oxygen?
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Which of the following correctly defines an element?
Which of the following correctly defines an element?
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What was the main concept of John Dalton's Atomic Theory?
What was the main concept of John Dalton's Atomic Theory?
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What is the correct interpretation of the term 'molecule'?
What is the correct interpretation of the term 'molecule'?
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Which of these is an example of a compound?
Which of these is an example of a compound?
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With respect to the subatomic particles, which statement is true?
With respect to the subatomic particles, which statement is true?
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Who is credited with proposing the Planetary Model of the atom?
Who is credited with proposing the Planetary Model of the atom?
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Which scientist first identified the proton?
Which scientist first identified the proton?
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What does the mass number of an element represent?
What does the mass number of an element represent?
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Which model proposed by Erwin Schrödinger describes electrons in a three-dimensional space?
Which model proposed by Erwin Schrödinger describes electrons in a three-dimensional space?
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What was a key change in the IUPAC numbering of the periodic table?
What was a key change in the IUPAC numbering of the periodic table?
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Which of the following best explains the purpose of the periodic table?
Which of the following best explains the purpose of the periodic table?
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What does the electron count in an atom equal when the atom is neutral?
What does the electron count in an atom equal when the atom is neutral?
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What was a significant limitation of the early classification of elements into metals and non-metals?
What was a significant limitation of the early classification of elements into metals and non-metals?
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What is the definition of atomic radius?
What is the definition of atomic radius?
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Which of the following describes ionization potential?
Which of the following describes ionization potential?
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What is electronegativity a measure of?
What is electronegativity a measure of?
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Which of the following elements belongs to the alkaline earth metals?
Which of the following elements belongs to the alkaline earth metals?
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Which principle states that no two electrons in an atom can have the same set of quantum numbers?
Which principle states that no two electrons in an atom can have the same set of quantum numbers?
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What does the Aufbau Principle dictate about electron configuration?
What does the Aufbau Principle dictate about electron configuration?
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Which group contains the halogens?
Which group contains the halogens?
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Which of the following describes electron affinity?
Which of the following describes electron affinity?
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What is the electron configuration for chromium (Cr)?
What is the electron configuration for chromium (Cr)?
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Which of the following elements has a fully-filled 3d subshell in its electron configuration?
Which of the following elements has a fully-filled 3d subshell in its electron configuration?
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When forming the cation V4+, which electrons are removed first from the electron configuration?
When forming the cation V4+, which electrons are removed first from the electron configuration?
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What is the electron configuration of V4+ after removing the required electrons?
What is the electron configuration of V4+ after removing the required electrons?
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What is the main characteristic of transition metals regarding their electron configurations?
What is the main characteristic of transition metals regarding their electron configurations?
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Which transition metal is specifically known for having a half-filled d subshell?
Which transition metal is specifically known for having a half-filled d subshell?
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In the electron configuration process for transition metals, where do electrons get removed first when forming cations?
In the electron configuration process for transition metals, where do electrons get removed first when forming cations?
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What is the noble gas shorthand notation for Vanadium (V)?
What is the noble gas shorthand notation for Vanadium (V)?
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Study Notes
Atoms, Elements and Compounds
- Atoms:
- Smallest unit of matter
- Contains protons, neutrons, and electrons
- Building blocks of matter
- Smallest part of an element
- Examples: Oxygen, Hydrogen, Nitrogen
- Elements:
- Pure substances made up of one type of atom
- Identified by atomic number (number of protons)
- Found on the Periodic Table of Elements
- Examples: Oxygen, Hydrogen, Nitrogen
- Molecules:
- Formed when two or more atoms join chemically
- Can be the same atoms (e.g., Oxygen molecule) or different atoms (e.g., Water)
- Compounds:
- Formed when two or more different elements join together
- All compounds are molecules but not all molecules are compounds
Atomic Theory
- Democritus proposed that matter is made of small indivisible particles called "atomos."
- John Dalton proposed the "Billiard Ball Model," where an atom is a hard, indestructible sphere.
- He also proposed the following atomic theory:
- Matter is made up of atoms.
- All atoms of a given element are alike.
- Atoms enter into combustion with other atoms to form compounds, but remain unchanged during ordinary chemical reactions.
- He also proposed the following atomic theory:
- J.J. Thomson discovered electrons and proposed the "Raisin Bread Model."
- This model suggested that electrons are embedded in a positively charged sphere.
- Eugen Goldstein identified "proton" but did not name it.
- Ernest Rutherford, through the "Gold Film Experiment," proved the presence of protons, coined the term "proton," and discovered that atoms are mostly empty space.
- Niels Bohr proposed the "Planetary Model," stating that electrons revolve around the nucleus in specific orbits.
- Erwin Schrödinger proposed the "Quantum Mechanic Model," also known as the "Electron Cloud Model," where electrons move around the nucleus in a 3D structure (orbitals).
- James Chadwick discovered the "neutron," which has no charge.
Element
- Atomic Number: Number of protons.
- Mass Number: Number of protons + neutrons.
- Neutron: Mass number - protons.
- Electron: Number of protons - charge.
Periodic Table of Elements
- Organizes chemical elements by increasing atomic number.
- Elements are arranged from left to right and top to bottom.
- Consists of 18 groups (columns) and 7 periods (rows).
- Divided into sections or blocks (s, p, d, f) representing energy sublevels.
- Used to summarize and predict element properties.
Periodic Classification of Elements
- Classification of elements: Arranging elements into groups based on property similarities.
- Makes studying elements easier.
- Early attempts at classification: Initial attempts involved grouping elements into metals and nonmetals.
- Limited because it did not account for metalloids.
- Antoine-Laurent Lavoisier grouped elements as metals and nonmetals in 1789.
- Johann Wolfgang Döbereiner classified elements into groups of three called "triads" based on similar properties and atomic mass.
- John A. Newlands arranged elements by increasing atomic mass and noticed a recurring pattern every eighth element, which he called the "Law of Octaves."
- Julius Lothar Meyer plotted a graph to group elements by atomic weight.
- Dimitri Mendeleev (father of the Periodic Table) arranged elements by increasing atomic weights, revealing a periodic repetition of properties.
- Henry Moseley discovered the modern Periodic Law: Element properties are a periodic function of their atomic number, not atomic weight.
Periodic Trends
- Atomic Radius: 1/2 distance between two nuclei.
- Metallic Property/Character: Level of reactivity of a metal.
- Ionization Potential: The minimum energy required to remove the most loosely bound electron (valence electron).
- Electron Affinity: Energy released or spent when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion.
- Electronegativity: The tendency of an atom to attract a bonding pair of electrons.
- Electropositivity: The tendency of atoms to lose electrons and form positive ions.
Groups / Families
- IA: Alkali Metals (H, Li, Na, K, Rb, Cs, Fr)
- IB: Coinage Metals (Cu, Ag, Au)
- IIA: Alkaline Earth Metals (Be, Mg, Ca, Sr, Ba, Ra)
- IIB: Zinc Family/Volatile Metals (Zn, Cd, Hg)
- IIIA: Boron Family/Icosagens (B, Al, Ga, In, Tl)
- IIIB: Scandium Subgroup (Sc, Y, Lanthanides, Actinides)
- IVA: Carbon Family/Crystallogens (C, Si, Ge, Sn, Pb)
- IVB: Titanium Subgroup (Ti, Zr, Hf)
- VA: Nitrogen Family/Pnictogens (N, P, As, Sb, Bi)
- VB: Vanadium Subgroup (V, Nb, Ta)
- VIA: Chalcogens/Oxygen Family (O, S, Se, Te, Po)
- VIB: Chromium Subgroup (Cr, Mo, W, U)
- VIIA: Halogens (F, Cl, Br, I, At)
- VIIB: Manganese Subgroup (Mn, Te, Re, Bh)
- VIIIA: Inert/Noble/Stable Gases (He, Ne, Ar, Kr, Xe, Rn)
- VIIIB: Iron Triads (Fe, Co, Ni), Palladium Triads (Rh, Ru, Pd), Platinum Triads (Os, Ir, Pt)
Quantum Mechanics
- Focuses on the behavior of electrons in atoms.
Principles of Electron Configuration
- Electron Configuration: Distribution of electrons in orbitals.
- Represents the location of electrons around the nucleus.
- Governed by these principles:
- Pauli's Exclusion Principle: Each atomic orbital can only have a maximum of 2 electrons, and these electrons must have opposite spin
- Aufbau's Principle: Electrons fill orbitals in order of increasing energy.
- Hund's Rule: When filling orbitals with the same energy level, electrons will occupy individual orbitals as much as possible before pairing in a single orbital.
Exceptions to Expected Electron Configurations
- Some exceptions to the order of filling orbitals occur for transition metals.
- Chromium (Cr) and Copper (Cu) prioritize half-filled and fully-filled 3d subshells.
Electron Configurations of Transitional Metal Ions
- Transition metals can exist in multiple oxidation states.
- When forming cations, electrons are removed from the highest energy shell first (4s before 3d, 5s before 4d, etc.)
Seatwork
- Find the long-hand electron configuration (expanded), noble gas electron configuration (shortened), and orbital notation/diagram for:
- Nickel (Ni)
- Nickel 2+ (Ni2+)
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Description
Test your knowledge of the basics of atomic theory, atoms, elements, molecules, and compounds. This quiz will cover key concepts and definitions that form the foundation of chemistry. Perfect for students learning about the building blocks of matter.
