General Chemistry - Matter and Atoms
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Questions and Answers

What is the main characteristic of an isobar?

  • Same mass number, different elements
  • Different atomic number, same mass number (correct)
  • Same atomic number, different mass number
  • Same element with different molecular structures

Which of the following best defines an allotrope?

  • Atoms in their simplest form
  • Atoms of the same element in different arrangements (correct)
  • Different isotopes of an element
  • Molecules composed of different elements

Who is credited with coining the term 'atomos'?

  • Aristotle
  • Newton
  • Plato
  • Democritus (correct)

Which two allotropes of carbon are commonly known?

<p>Diamond and Graphite (B)</p> Signup and view all the answers

What distinguishes isotopes from isobars?

<p>Isotopes have the same number of protons (A)</p> Signup and view all the answers

Which statement is true regarding isomers?

<p>Isomers have identical molecular formulas but different structures (A)</p> Signup and view all the answers

What does 'alotropism' refer to?

<p>The ability of an element to exist in multiple forms (A)</p> Signup and view all the answers

Which is true about isotones?

<p>They have the same number of neutrons (B)</p> Signup and view all the answers

What model did John Dalton propose regarding the structure of atoms?

<p>The Billiard Ball Model (C)</p> Signup and view all the answers

According to Dalton's Atomic Theory, which of the following statements is true?

<p>Atoms combine in simple numerical ratios. (D)</p> Signup and view all the answers

What is the azimuthal quantum number (l) used to determine?

<p>The shape of the orbital (A)</p> Signup and view all the answers

What is the principal quantum number (n) associated with?

<p>The size of the particle (C)</p> Signup and view all the answers

Which of the following statements accurately characterizes John's view on atoms?

<p>Atoms remain unchanged during ordinary reactions. (D)</p> Signup and view all the answers

In the 'Raisin Bread Model' proposed by J.J. Thompson, what does the 'bread' represent?

<p>Positively charged particles (A)</p> Signup and view all the answers

What does the magnetic quantum number (M or $m_l$) indicate?

<p>Orientation of the orbital (C)</p> Signup and view all the answers

Which statement correctly reflects the concept of atoms according to traditional atomic theory?

<p>Atoms can combine to form many different compounds. (D)</p> Signup and view all the answers

What is the molar mass of Magnesium Oxide (MgO)?

<p>40 g/mole (D)</p> Signup and view all the answers

Which principle states that no two electrons can have the same set of quantum numbers?

<p>Pauli’s Exclusion Principle (C)</p> Signup and view all the answers

According to Heisenberg's Uncertainty Principle, what aspect of electrons cannot be accurately determined at the same time?

<p>Position and momentum (D)</p> Signup and view all the answers

What does Hund’s Rule of Maximum Multiplicity state about orbital filling?

<p>All orbitals in a sublevel must be filled before pairing occurs (C)</p> Signup and view all the answers

Which scientist is known as the 'Father of the Modern Periodic Table'?

<p>Dmitri Mendeleev (D)</p> Signup and view all the answers

What does the Law of Triads, proposed by John Wolfgang Dobereiner, explain?

<p>Elements can be grouped in threes based on atomic weight (C)</p> Signup and view all the answers

Which principle explains the filling order of electrons in atomic orbitals?

<p>Aufbau's Building Up Principle (C)</p> Signup and view all the answers

Henry Moseley's work led to the creation of which important concept in the periodic table?

<p>Properties vary with increasing atomic number (B)</p> Signup and view all the answers

What is the process of transforming a gas directly into a solid called?

<p>Deposition (A)</p> Signup and view all the answers

Which of the following is NOT considered evidence of a chemical change?

<p>Phase change without new substance (C)</p> Signup and view all the answers

What is produced when an alkaline reacts with fat in the saponification process?

<p>Glycerol (A)</p> Signup and view all the answers

In a single displacement reaction, which of the following represents the correct formula?

<p>AB + C → AC + B (B)</p> Signup and view all the answers

Nuclear fission is best described as the...

<p>Splitting of a heavy atom into smaller nuclei (C)</p> Signup and view all the answers

Which of the following describes a direct union or combination reaction?

<p>A + B → AB (D)</p> Signup and view all the answers

What type of reaction is fermentation classified as?

<p>Chemical change (B)</p> Signup and view all the answers

In which reaction does a compound break down into simpler substances?

<p>Decomposition reaction (D)</p> Signup and view all the answers

What is the general representation of a double displacement reaction?

<p>AB + CD → AC + BD (C)</p> Signup and view all the answers

What type of reaction occurs in neutralization?

<p>Acid + Base → Salt + Water (B)</p> Signup and view all the answers

Which of the following describes a homogenous mixture?

<p>Uniform mixture with one phase (D)</p> Signup and view all the answers

Which process involves the addition of oxygen?

<p>Oxidation (B)</p> Signup and view all the answers

What type of mixture is described as a suspension?

<p>Liquid containing insoluble solid particles (A)</p> Signup and view all the answers

Which method is specifically used for separating magnetic materials?

<p>Magnetic Separation (D)</p> Signup and view all the answers

Hydrolysis can be represented by which of the following reactions?

<p>H2O + Salt → Acid + Base (D)</p> Signup and view all the answers

In a double displacement reaction, which statement is true?

<p>Two reactants exchange components. (C)</p> Signup and view all the answers

What is the main principle behind the process of decantation?

<p>Difference in specific gravity/density (A)</p> Signup and view all the answers

Which of the following best describes a colloid?

<p>Particles that remain suspended and evenly disperse throughout a medium (A)</p> Signup and view all the answers

What is a key factor to ensure when using a centrifuge?

<p>Ensure the machine is balanced by adding samples directly across from each other (A)</p> Signup and view all the answers

In fractional crystallization, what happens as the temperature is lowered?

<p>Less soluble components crystallize first (A)</p> Signup and view all the answers

Which method is most commonly used for chromatographic separation?

<p>Paper chromatography (D)</p> Signup and view all the answers

What is the main effect of centrifugation on a mixture?

<p>It speeds up the settling process of precipitates (A)</p> Signup and view all the answers

What characteristic limits the size of solute particles in a colloid?

<p>They must remain suspended but not settle (D)</p> Signup and view all the answers

What is the purpose of the supernatant liquid in decantation?

<p>To be poured out, leaving precipitates behind (A)</p> Signup and view all the answers

Flashcards

Chemical Change

A change in both intrinsic and extrinsic properties of a substance.

Direct Union (Combination/Synthesis)

Two or more substances combine to form a new substance.

Decomposition

A single substance breaks down into two or more simpler substances.

Single Replacement

One element replaces another element in a compound.

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Saponification

The process that produces soap. An alkaline substance reacts with fat to make soap and glycerol.

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Nuclear Change

A change in the structure, properties, and composition of an atom's nucleus.

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Nuclear Fission

The splitting of a heavy atom into smaller atoms.

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Nuclear Fusion

The combining of light atoms into a heavier atom.

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Double Displacement

A chemical reaction where two reactants exchange parts to form two new products. It often involves the swapping of ions between two compounds.

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Neutralization

A specific type of double displacement reaction where an acid and a base react to form salt and water.

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Oxidation

A chemical reaction where an element gains oxygen atoms.

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Reduction

A chemical reaction where an element loses oxygen atoms or gains hydrogen atoms.

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Hydrolysis

A chemical reaction where water breaks down a compound into two or more other components.

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Homogeneous Mixture

A mixture where the components are evenly distributed and have a uniform appearance.

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Heterogeneous Mixture

A mixture where the components are not evenly distributed and have a non-uniform appearance.

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Solution

A type of homogeneous mixture where a solute (substance that dissolves) is evenly distributed in a solvent (substance that dissolves the solute).

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Colloid

A mixture where particles are larger than molecules but small enough to stay suspended, giving a uniform appearance.

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Decantation

Separating a liquid from a solid by carefully pouring off the liquid, leaving the solid behind.

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Centrifugation

Spinning a mixture at high speed to separate components based on density. Heavier particles move to the bottom.

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Fractional Crystallization

Separating components by controlling temperature. The least soluble component crystallizes first.

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Chromatography

Separating components by their different attractions to a stationary phase and a mobile phase.

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Paper Chromatography

A specific type of chromatography where a stationary phase is paper and a mobile phase is a solvent.

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What is the purpose of a centrifuge?

To speed up the settling process of a precipitate by applying centrifugal force.

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Why is it important to balance a centrifuge?

To prevent the centrifuge from shaking or vibrating excessively, potentially causing damage or accidents.

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Atomos

The term coined by Democritus for the smallest, indivisible particles that make up matter. It means "indivisible" in Greek.

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Democritus's Contribution

Democritus was a Greek philosopher who proposed the idea that matter is made up of small, indivisible particles called atoms. He emphasized the importance of observation and experimentation.

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Isotopes

Isotopes are atoms of the same element that have the same number of protons (atomic number) but different numbers of neutrons, resulting in different mass numbers.

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Isotones

Isotones are atoms of different elements that have the same number of neutrons but different numbers of protons and, therefore, different atomic numbers.

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Isobars

Isobars are atoms of different elements that have the same mass number but different numbers of protons and neutrons.

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Isomers

Isomers are molecules that have the same molecular formula (same types and numbers of atoms) but different structural arrangements, leading to different properties.

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Allotropes

Allotropes are different forms of the same element in the same physical state (solid, liquid, or gas) but have different arrangements of atoms, resulting in different properties.

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Allotropes of Carbon

Diamond and graphite are allotropes of carbon, meaning they are both made of carbon atoms but arranged differently, leading to their distinct properties.

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Dalton's Atomic Theory

A set of ideas about the nature of matter, stating that matter is composed of tiny, indivisible particles called atoms. All atoms of a given element are identical, and atoms can combine in simple numerical ratios to form compounds.

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Billiard Ball Model

Dalton's model of the atom, depicting it as a hard, indestructible sphere, similar to a billiard ball.

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What did Dalton's Atomic Theory disprove?

Dalton's theory disproved the idea that atoms can be further divided into smaller particles. Later discoveries revealed the existence of subatomic particles.

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What is a nascent species?

A species of a chemical element in its atomic form, meaning it is not bonded to any other atoms. It is highly reactive and short-lived.

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What is a molecular species?

A species of a chemical element where two or more atoms are bound together. They are relatively stable and have different properties than their atomic form.

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Principal Quantum Number (n)

A quantum number that describes the main energy level or shell of an electron in an atom. It determines the size and energy of the electron's orbital.

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Azimuthal or Angular Momentum Quantum Number (l)

A quantum number that describes the shape of an electron's orbital in an atom. It determines the subshell or sublevel, with values ranging from 0 to (n-1).

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Magnetic Quantum Number (ml or m)

A quantum number that describes the orientation of an electron's orbital within a subshell. It determines the specific orbital within a subshell, with values ranging from -l to +l.

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Pauli Exclusion Principle

No two electrons in an atom can have the same set of four quantum numbers.

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Heisenberg Uncertainty Principle

It's impossible to simultaneously determine an electron's exact momentum (speed and direction) and its position.

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Aufbau Principle

Electrons fill lower energy levels before filling higher ones.

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Hund's Rule

Electrons fill orbitals singly before pairing up within the same subshell.

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Antoine Lavoisier

Created the first extensive list of 33 elements, distinguishing metals from nonmetals.

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Dobereiner's Law of Triads

Groups of three elements with similar chemical properties, where the middle element's atomic mass is the average of the other two.

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Newlands' Law of Octaves

Every eighth element had similar properties, resembling musical octaves.

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Mendeleev's Contribution

Organized the periodic table by atomic mass and predicted the existence of undiscovered elements.

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Study Notes

Module I: General Chemistry - Course Audit I

  • This module covers General Chemistry topics.
  • The course audit includes 15 pages of material.
  • Covered topics include: Matter, Atoms, Fundamental Chemistry Laws, Periodic Table of Elements, Kinetic Molecular Theory, Acids and Bases.

Topic 1: Matter

  • Matter: Anything occupying space and having mass.
  • Classification of Matter:
    • Elements: Simplest form, single component.
    • Compounds: Two or more elements combined chemically.
    • Mixtures: Two or more substances not chemically combined.
  • Mass vs Weight: Mass measures quantity of particles, weight is the force due to gravity.
  • States of Matter: Solid, Liquid, Gas.

Topic 2: Atoms

  • Atomic Structure: Protons, Neutrons, Electrons.
  • Atomic Number: Number of protons.
  • Mass Number: Sum of protons and neutrons.
  • Electron Cloud: Describes the structure of an atom.
  • Electron arrangement: Lower energy levels filled first.
  • Quantum Numbers: Used to describe electron properties.
  • Atomic Models: Billiard ball model, raisin bread model, planetary model, electron cloud model.

Topic 3: Fundamental Chemistry Laws

  • Law of Conservation of Mass (Lavoisier): Mass is neither created nor destroyed.
  • Law of Definite Proportions (Proust): Compounds have fixed mass ratios.
  • Law of Multiple Proportions (Dalton): Elements can combine in different ratios to form more than one compound.
  • Law of Combining Weights (Dalton): The proportions of reacting elements are fixed.

Topic 4: The Periodic Table of Elements

  • Periodic Trends:
    • Atomic radius: Increases down and left on the table.
    • Ionization energy: Increases up and right.
    • Electronegativity: Increases up and right.
    • Metallic character: Increases down and left.
  • Electron Configuration: Arrangement of electrons in atomic orbitals explains periodic trends.
  • Important Scientists: Lavoisier, Döbereiner, Newlands, Mendeleev, Moseley, Seaborg, and others contributed to the development of the table
  • Useful Trivias: Most abundant elements, first artificially produced element, rarest element etc.
  • Periodic Table Families: Representative elements (A), Transition elements (B).

Topic 5: Kinetic Molecular Theory

  • Kinetic Molecular Theory Explains states of matter based on the movement of particles.
  • Explains differences between solid, liquid, gas phases.
  • Factors affecting solubility: Nature of solute and solvent (like dissolves like), temperature (↑ temp ↑ solubility), pressure (↑ pressure ↑ solubility for gases), particle size/surface area (smaller particles more soluble), presence of salts.

Topic 6: Acids and Bases

  • Acids and Bases:
    • Acids: Sour taste, turn blue litmus red, react with metals.
    • Bases: Bitter taste, turn red litmus blue, often soapy to the touch.
  • Electrolytes: Strong vs. weak.
  • Acid-Base Theories: Arrhenius, Brønsted-Lowry, Lewis.
  • pH: Measure of acidity or basicity.
  • Buffers: Resist changes in pH.

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This quiz covers foundational concepts in General Chemistry, focusing on Matter and Atoms. Learn about the classification of matter, the atomic structure, and fundamental chemistry laws that govern these topics. Ideal for anyone looking to audit their knowledge in Chemistry.

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