Chemistry Chapter 4 Review Flashcards

Questions and Answers

Who was the first to refer to the smallest particles composing matter as atoms?

Democritus

What states that it is impossible to know both the energy level and the exact position of an electron at the same time?

Heisenberg Uncertainty Principle

A type of sublevel found in all principle energy levels is the...

Which atomic model helped explain line spectra?

Bohr's model of the atom Signup and view all the answers

The sum of the number of neutrons and the number of protons in the nucleus of an atom is...

mass number (atomic mass) Signup and view all the answers

Which principle describes how electrons fill orbitals?

Aufbau principle Signup and view all the answers

What states that atoms of each element have unique sizes and properties?

Dalton's atomic model Signup and view all the answers

What states that any sample of water always contains 8 g of oxygen for every 1 g of hydrogen?

law of definite composition Signup and view all the answers

Who discovered x-rays?

William Roentgen Signup and view all the answers

What describes how electrons fill a sublevel?

Hund's rule Signup and view all the answers

Who developed cathode rays?

J.J. Thomson Signup and view all the answers

Who developed the first atomic model?

John Dalton Signup and view all the answers

What is a negatively charged ion?

anion Signup and view all the answers

Who first stated the discontinuity of matter?

Democritus Signup and view all the answers

Who is responsible for proposing the wave nature of the electron?

Broglie Signup and view all the answers

Which subatomic particle has the greatest atomic mass?

neutron Signup and view all the answers

Two electrons located in the same orbital have opposite spins is the...

Pauli exclusion principle Signup and view all the answers

Who discovered neutrons?

Chadwick Signup and view all the answers

Who developed the uncertainty principle?

Heisenberg Signup and view all the answers

Who discovered protons?

Rutherford Signup and view all the answers

Who discovered the prism spectroscope?

Kirchoff and Bunsen Signup and view all the answers

Write the isotopic notation for sodium.

23Na Signup and view all the answers

Explain how atoms can be electrically neutral even though they contain charged particles.

Equal number of protons and electrons neutralize each others' charges Signup and view all the answers

Describe what happens to the outermost electron when a sodium atom is heated and made to give off a line spectrum.

The electron gains energy, jumps to a higher orbital and then returns to a lower orbital, releasing the excess energy as light. Signup and view all the answers

What is the electron capacity for the s sublevel?

2 Signup and view all the answers

What is the electron capacity for the p sublevel?

6 Signup and view all the answers

What is the electron capacity for the d sublevel?

10 Signup and view all the answers

What is the electron capacity for the f sublevel?

14 Signup and view all the answers

What new technique do scientists use in order to image (see) atoms?

scanning tunneling microscope Signup and view all the answers

How many valence electrons for barium?

2 Signup and view all the answers

How many valence electrons for phosphorus?

5 Signup and view all the answers

How many valence electrons for krypton?

8 Signup and view all the answers

State Dalton's atomic theory (3).

<ol> <li>Elements are composed of tiny, indestructible spheres. 2. Atoms form compounds by combining with each other. 3. Atoms of one element cannot be changed into atoms of another element.</li> </ol> Signup and view all the answers

Study Notes

Atomic Concepts and Theories

Democritus first identified atoms as the fundamental particles of matter.
Dalton's atomic theory posits that elements consist of indestructible spheres, atoms combine to form compounds, and atoms of one element cannot transform into those of another element.
Heisenberg Uncertainty Principle indicates simultaneous uncertainty in an electron's energy level and exact position.

Atomic Structure

The mass number is the sum of neutrons and protons in an atom's nucleus.
Anions are negatively charged ions formed when atoms gain electrons.
Neutrons have the greatest atomic mass among subatomic particles.

Electron Configuration Principles

The Aufbau principle describes the order in which electrons fill orbitals.
Hund's rule states that electrons occupy each orbital singly before pairing up.
Pauli exclusion principle asserts that no two electrons in the same orbital can have identical spins.

Electron Sublevels and Capacities

The s sublevel can hold up to 2 electrons.
The p sublevel has a capacity of 6 electrons.
The d sublevel accommodates 10 electrons.
The f sublevel can hold 14 electrons.

Historical Contributions

John Dalton developed the first atomic model.
J.J. Thomson created cathode rays and discovered electrons.
Ernest Rutherford discovered protons through his experiments.
James Chadwick identified neutrons.
William Roentgen discovered x-rays, expanding the understanding of atomic particles.

Spectroscopy and Light Emission

Bohr's model effectively explains the emission spectra of atoms.
Heating a sodium atom causes the outermost electron to absorb energy, jump to a higher orbital, and release light upon returning to a lower orbital.
The law of definite composition indicates that a specific ratio of elements is always present in a compound, such as water containing 8 g of oxygen for every 1 g of hydrogen.

Advanced Imaging and Techniques

A scanning tunneling microscope is a modern tool used to visualize atomic structures accurately.

Valence Electrons

Barium has 2 valence electrons.
Phosphorus possesses 5 valence electrons.
Krypton has a full complement of 8 valence electrons.

Isotopic Notation

The isotopic notation for sodium is represented as (^{23}_{11}Na).

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Test your knowledge and understanding of key concepts from Chemistry Chapter 4 with these flashcards. This quiz covers important terms and principles related to atomic theory and electron behavior. Perfect for students preparing for exams!