Chemistry Solutions and Matter Classification

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Questions and Answers

Which term describes a solution that contains the maximum amount of solute that can be dissolved at a given temperature?

Unsaturated

Saturated (correct)

Supersaturated

Dilute

Which of the following is an example of a physical change?

Rust forming on iron

Cooking an egg

Burning a piece of wood

Dissolving sugar in water (correct)

What type of property does density represent?

Intensive property (correct)

Extensive property

Qualitative property

Chemical property

Which term is used to describe a solution with very little solute present?

Unsaturated Signup and view all the answers

Which of the following is a qualitative measurement?

Color Signup and view all the answers

What occurs in a supersaturated solution?

There is more solute than can be dissolved. Signup and view all the answers

Which term describes the smallest unit of an element that retains all chemical properties of that element?

Atom Signup and view all the answers

Which of the following best defines an extensive property?

Is dependent on the size of the sample Signup and view all the answers

What does the Law of Conservation of Mass state?

Mass remains constant in a chemical reaction. Signup and view all the answers

According to Dalton’s Atomic Theory, what is the fundamental unit of matter?

Atom Signup and view all the answers

Which of the following is an example of an extensive property?

Mass Signup and view all the answers

What happens during an extensive change?

New substances are created that are entirely different from the original. Signup and view all the answers

What did J.J. Thomson discover about cathode rays?

They are made of negatively charged particles that are lighter than atoms. Signup and view all the answers

Which principle states that compounds contain the same elements in the same proportion by mass?

Law of Definite Composition Signup and view all the answers

What characteristic is NOT a result of an extensive change?

No new substances are formed Signup and view all the answers

Who first proposed that electricity consists of particles?

Michael Faraday Signup and view all the answers

What is the shape of the s orbital?

Spherical Signup and view all the answers

What criteria differentiates compounds from mixtures?

Compounds are composed of two or more elements chemically combined. Signup and view all the answers

Which sublevel can accommodate the maximum number of electrons?

f sublevel Signup and view all the answers

Which of the following statements about homogenous mixtures is true?

They have uniform composition throughout. Signup and view all the answers

What do arrows represent in an orbital diagram?

Unpaired electrons Signup and view all the answers

What is the significance of the law of definite proportions in a compound?

A compound always contains its elements in a fixed ratio. Signup and view all the answers

Which is true about the electron configuration in relation to the periodic table?

Column numbers reflect the number of electrons allowed in each sublevel. Signup and view all the answers

Why do compounds differ from diatomic molecules?

Compounds consist of more than two different elements. Signup and view all the answers

What is the correct order of energy levels for atomic orbitals?

s, p, d, f Signup and view all the answers

What can the Tyndall effect indicate in a solution?

The particles are smaller than the wavelength of visible light. Signup and view all the answers

Who proposed the Nuclear Model of the atom, which includes a small positively charged nucleus?

Ernest Rutherford Signup and view all the answers

What is an isotope?

Atoms of the same element that differ in mass. Signup and view all the answers

In the Modern Atomic Model, which of the following describes the primary role of the principal energy level?

It shows how far the orbital extends from the nucleus. Signup and view all the answers

Which sublevel can contain a maximum of six electrons?

p Signup and view all the answers

Which model describes electrons as being in fixed orbits around the nucleus?

Planetary Model Signup and view all the answers

What did Niels Bohr contribute to the understanding of atomic structure?

He emphasized stability of electrons in quantized orbits. Signup and view all the answers

What is the primary discovery attributed to James Chadwick in 1932?

The discovery of neutron in the nucleus. Signup and view all the answers

Which model gives a probability map for where an electron might be found in an atom?

Quantum Mechanical Model Signup and view all the answers

Which sublevel has the highest electron capacity?

f Signup and view all the answers

In Schrodinger's model, which aspect of electrons is described as uncertain?

Their location or momentum. Signup and view all the answers

Study Notes

Homogenous (solution)

Uniform composition
Solute dissolves in solvent
Solvents can be solid, liquid, or gas
Examples: sugar water, salt water, gasoline

Solution Types

Saturated: Correct amount of solute in solvent
Unsaturated: Very few solute in solvent
Supersaturated: Too much solute in solvent

Classification of Matter

Systematic way of determining classification using properties of matter
Change Involved During Measurement
- Physical Change
  - Characteristic that can be observed without changing composition.
  - Involves physical change like shape, size, and state.
  - Qualitative: Color, odor.
  - Quantitative: Mass, Volume, Density, Temperature
- Chemical Change
  - Composed of 2 or more elements chemically combined in definite proportions.
  - Examples: Water, sugar, salt
  - Acids: Less than pH 7
  - Bases: Greater than pH 7
  - Salts: Combination of Acids and Bases
  - Compounds: Often have to be different elements. Diatomic does not equal a compound.
Amount of Matter During Measurement
- Intensive property: Characteristic that does not change value when the amount of substance is changed.
  - Examples: Color, Density, Boiling point, Melting point
- Extensive Property: Characteristic that changes value as the amount of substance is changed
  - Examples: Volume, Mass, Weight, Length

Mixtures

Combination of two or more (pure) elements/compounds

Development of Atomic Theory

Law of Conservation of Mass: Mass cannot be created nor destroyed (Antoine Lavoisier, 1789)
Law of Definite Composition: Compounds contain the same elements in exactly the same proportion by mass (Joseph Proust, 1799)
Dalton’s Atomic Theory: Matter is composed of atoms, and elements are composed of identical atoms (John Dalton, 1808)
- Matter is composed of small, indivisible particles called atoms.
- All atoms of a given element are identical both in mass and in chemical properties.
- Atoms of different elements have different masses and different chemical properties.

Atom and its Properties

"Atomos" = “indivisible”
The smallest unit of an element that retains all chemical properties of an element.
Leucippus and Democritus agreed that they are composed of small, finite particles.
Aristotle’s idea that they were made up of elements stayed for up to 2000 years.
Molecules:
- Criteria:
  - Does not spontaneously separate or settle out over time.
  - Tyndall effect can be observed by eye (nanometer-sized particles)
  - Tyndall effect: Particles of solute and solvent are smaller than the wavelength of the visible light.
Law of definite proportions: Given chemical compound always contains its component elements in a fixed ratio regardless the substance’s mass.

Subatomic Particles

Michael Faraday (1834): Electricity consists of particles.
George J.Stoney (1874): Electrons (unit of electrical charge) are exchanged in electro-chemical reactions.
William Crookes (1879): Cathode rays are made of charged atoms.
J.J Thomson (1897): Cathode rays are made of particles lighter than atoms and can be deflected by an negative electric field. Atoms are divisible. Corpuscles (negatively charged subatomic particles) are building blocks.
Discovery of the Electron
- Cathode Ray generates electrons. A small, relatively heavy, and positively charged body (the nucleus) must be at the center of each atoms. (Ernest Rutherford, 1907)
Plum Pudding Model
- Negatively-charged electrons in a positively-charged sphere.
Nuclear Model
- Small positively charged nucleus (most of the mass is in the nucleus). Rutherford discovered that the nuclei of other elements contain hydrogen nucleus as a building block named the proton.
Isotopes: Atoms of the same element that differ in mass.

Neils Bohr (1913)

Planetary Model
- Electrons in orbit around a nucleus (account for stability of electrons)

Erwin Schrodinger & Werner Heisenberg (1913)

Quantum Mechanical Model (accepted)
- Electrons most probably in this region (uncertainty in location or momentum of electrons)

James Chadwick (1932)

Discovered the Neutron
- There are neutrons in the nucleus.
- Atoms have a nucleus that contains protons and neutrons (electrons move around the nucleus)

Modern Atomic Model

Based on Schrodinger’s mathematical model of waves: probability map of where electron is found.
Orbitals: 3D region in space where electrons are likely to be found.
Principal Energy level: As this energy level increases, the orbital extends further from the nucleus.
- n = 1: One 1s orbital = 2 electrons
- n = 2: 2s orbital and three 2p orbitals = 8 electrons
- n = 3: 3s orbital, three 3p orbitals, and five 3d orbitals = 18 electrons
- n = 4: 4s orbital, three 4p orbitals, five 4d orbitals, & seven 4f orbitals = 32 electrons
Sublevels
- s: Spherical = 2 electrons
- p: Dumbbell = 6 electrons
- d: Clover = 10 electrons
- f: Flower = 14 electrons

Electron Configuration of the Periodic Table

Number of the column in the s, p, d, and f blocks is the same as the number of electrons allowed in each sublevel.
Number of columns = number of electrons allowed in each sublevel

Orbital Diagram

Diagram that represents the electronic structure of an atom.
Arranged according to energy levels:
- Electrons are represented by up and down arrows.
- Order of energy level of orbitals: s, p, d, f.
Hund’s Rule: Electrons are added to a shell in a way to give the maximum number of unpaired electrons.

Electron Configuration

Electronic configuration of the periodic table.

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Explore the properties of homogenous solutions and the classification of matter in this engaging quiz. Learn about saturated, unsaturated, and supersaturated solutions, as well as physical and chemical changes crucial to understanding chemistry. Test your knowledge about solutes, solvents, and measurement properties.