Chemistry Chapter 5 Flashcards
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Questions and Answers

An orbital can at most hold how many electrons?

2 electrons

How many electrons can the first energy level hold?

2

What are the sublevels that make up the n=3 energy level?

s, p, d

How many orbitals are in a 'p' sublevel?

<p>3</p> Signup and view all the answers

What is the Pauli Exclusion Principle?

<p>An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins</p> Signup and view all the answers

Which scientist developed the Quantum Mechanical Model?

<p>E. Schrödinger</p> Signup and view all the answers

How many electrons can the d sublevel hold?

<p>10</p> Signup and view all the answers

What is the lowest energy state of an atom called?

<p>ground state</p> Signup and view all the answers

How many electrons can the s sublevel hold?

<p>2</p> Signup and view all the answers

What orbital shapes are found at the 2nd energy level?

<p>s and p</p> Signup and view all the answers

What atom matches this electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10?

<p>zinc</p> Signup and view all the answers

What is the maximum number of electrons that an orbital can have?

<p>2 electrons</p> Signup and view all the answers

What electron configuration matches an oxygen atom?

<p>1s2 2s2 2p4</p> Signup and view all the answers

What is the electron configuration for Bromine (Br)?

<p>1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5</p> Signup and view all the answers

What is the shorthand electron configuration for a sulfur atom?

<p>[Ne] 3s2 3p4</p> Signup and view all the answers

Hund's rule states...

<p>Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.</p> Signup and view all the answers

Sublevel with a single orbital shaped like a sphere.

<p>s</p> Signup and view all the answers

When doing orbital diagrams, the large numbers (e.g. 1s, 2s) represent...

<p>energy levels</p> Signup and view all the answers

Name the element represented by the electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1.

<p>Gallium</p> Signup and view all the answers

How many electrons can a d sublevel hold?

<p>10</p> Signup and view all the answers

Used the 'Cathode Ray Tube Experiment' to make his discovery.

<p>Thomas</p> Signup and view all the answers

How many electrons can fit in a 'p' sublevel?

<p>6</p> Signup and view all the answers

Which is the electron configuration for an oxygen atom?

<p>1s2 2s2 2p4</p> Signup and view all the answers

What are the shapes of p orbitals?

<p>dumbbells</p> Signup and view all the answers

The electron configuration of an atom is 1s2 2s2 2p6. The number of electrons in the atom is...

<p>10</p> Signup and view all the answers

How many electrons can an f sublevel hold?

<p>14</p> Signup and view all the answers

What atom matches this electron configuration: 1s2 2s2 2p6 3s2?

<p>Magnesium</p> Signup and view all the answers

Sublevel with a set of 3 dumbbell shaped orbitals.

<p>p</p> Signup and view all the answers

How many electrons can an s sublevel hold?

<p>2</p> Signup and view all the answers

What are the sublevels that make up the n=4 energy level?

<p>s, p, d, f</p> Signup and view all the answers

Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?

<p>Aufbau Principle</p> Signup and view all the answers

λ is the symbol for which part of a wave?

<p>wavelength</p> Signup and view all the answers

The area of 3D space where an electron is likely to be found is called a(n)...

<p>orbital</p> Signup and view all the answers

ν is the symbol for which part of the wave?

<p>frequency</p> Signup and view all the answers

The height of a wave is called...

<p>amplitude</p> Signup and view all the answers

According to the Aufbau Principle, which sublevel should start filling with electrons after 5s?

<p>4d</p> Signup and view all the answers

Electron arrangement that uses arrows is called...

<p>orbital diagram</p> Signup and view all the answers

Atoms that gain & lose electrons are called...

<p>ions</p> Signup and view all the answers

What is the number of valence electrons for Carbon?

<p>4</p> Signup and view all the answers

This 'rule' of Quantum Chemistry states that no 2 electrons in an atom can be in the exact same state...

<p>Pauli Exclusion Principle</p> Signup and view all the answers

Which of the following is a p block element?

<p>Ar</p> Signup and view all the answers

Study Notes

Electron Configuration and Atomic Orbitals

  • Maximum capacity of an orbital is 2 electrons.
  • First energy level can hold 2 electrons.
  • n=3 energy level consists of s, p, and d sublevels.
  • p sublevel contains 3 orbitals, accommodating a total of 6 electrons.
  • d sublevel can hold up to 10 electrons, with 5 orbitals present for electron distribution.
  • f sublevel has a capacity of 14 electrons.

Principles Governing Electron Behavior

  • Pauli Exclusion Principle: No two electrons can occupy the same quantum state; at most 2 electrons can fit in one orbital with opposite spins.
  • Hund's Rule: Electrons fill degenerate orbitals singly first, ensuring the same spin until all orbitals in the energy level contain one electron.
  • Aufbau Principle: Electrons occupy the lowest energy orbitals first.

Orbital Shapes and Energy Levels

  • s sublevel has a spherical orbital shape, with 1 orbital available.
  • p orbitals have a dumbbell shape, consisting of 3 orbitals in a sublevel.
  • There are 4 sublevels in the n=4 energy level: s, p, d, and f.

Electron Configuration Examples

  • Zinc: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰.
  • Oxygen: 1s² 2s² 2p⁴.
  • Bromine: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵.
  • Gallium: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p¹.
  • Chlorine: 1s² 2s² 2p⁶ 3s² 3p⁵.
  • Aluminum: 1s² 2s² 2p⁶ 3s² 3p¹.
  • Manganese: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵.
  • Magnesium: 1s² 2s² 2p⁶ 3s².

Valence Electrons and Atomic Structure

  • Group 16 elements possess 6 valence electrons.
  • Carbon has 4 valence electrons.
  • Atomic orbitals are regions in space where electrons are likely to be found.

Wave Properties

  • Wavelength (λ) and frequency (ν) are fundamental wave characteristics; amplitude describes the wave's height.
  • Electrons and their energy states are represented and visualized in orbital diagrams, which utilize arrows to denote electron arrangements.

Historical Contributions

  • E. Schrödinger contributed to the development of quantum mechanics.
  • J.J. Thomson utilized the Cathode Ray Tube Experiment to discover the electron.

Quantum Chemistry Principles

  • Heisenberg Uncertainty Principle states that it is impossible to precisely know both the location and momentum of an electron simultaneously.

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Test your knowledge of Chemistry Chapter 5 with these flashcards. Focus on key concepts such as orbitals, energy levels, and principles like the Pauli Exclusion Principle. Perfect for students needing a quick review or study aid.

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