Chemistry Chapter 5: Electrons in Atoms
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Questions and Answers

Electromagnetic radiation is a kind of ______ that behaves like a(n) ________ as it travels through space.

Electromagnetic radiation is a kind of ______ that behaves like a(n) ________ as it travels through space.

Electromagnetic radiation is a kind of ______ that behaves like a(n) ________ as it travels through space.

energy, wave

What is one type of electromagnetic radiation?

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

All waves can be characterized by their wavelength, amplitude, frequency, and ______.

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

The shortest distance between equivalent points on a continuous wave is called a(n) ______.

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

The height of a wave from the origin to a crest or from the origin to a trough is the ______.

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

____ is the _______, which is equivalent to one wave per second.

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

What is the minimum amount of energy that can be lost or gained by an atom?

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

According to Planck's theory, for a given frequency, v, matter can emit or absorb energy on in ______.

<p>whole-number multiples of hv</p> Signup and view all the answers

What is the phenomenon where electrons are emitted from a metal's surface when light shines on it?

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

Which equation is used to calculate the energy of a photon?

<p>E = hv (Planck's constant)</p> Signup and view all the answers

Like the visible spectrum, an atomic emission spectrum is a continuous range of colors.

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

Each element has a unique atomic emission spectrum.

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

A flame test can be used to identify the presence of certain elements in a compound.

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

The fact that only certain colors appear in an element's atomic emission spectrum indicates that only certain frequencies of light are emitted.

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

Atomic emission spectra can be explained by the wave model of light.

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

The neon atoms in a neon sign emit their characteristic color of light as they absorb energy.

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

When an atom emits light, protons having certain specific energies are being emitted.

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

The lowest allowable energy state of an atom is called _______.

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

What did Bohr's model predict about hydrogen's atomic emission?

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

According to Bohr's atomic model, the smaller an electron's orbit, the ______ the atom's energy level.

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

Bohr proposed that when energy is added to a hydrogen atom, its ____ moves to a higher-energy orbit.

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

According to Bohr's atomic model, the hydrogen atom emits a photon corresponding to the difference between the _____ associated with the two orbits it transitions between.

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

What aspect of Bohr's model failed to explain elements other than hydrogen?

<p>atomic emission spectrum</p> Signup and view all the answers

What is the modern model of the atom that treats electrons as waves called?

<p>quantum mechanical model</p> Signup and view all the answers

What principle states it is impossible to know both the velocity and the position of a particle at the same time?

<p>Heisenberg uncertainty principle</p> Signup and view all the answers

What is a three-dimensional region around the nucleus representing the probability of finding an electron called?

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

Which equation was originally applied to the hydrogen atom and led to the quantum mechanical model?

<p>Schrodinger wave equation</p> Signup and view all the answers

Do atomic orbitals have an exact defined size?

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

Each orbital contains at most how many electrons?

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

All s orbitals are shaped this way.

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

A principal energy is represented by what variable?

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

What does 2n squared find?

<p>max number of electrons</p> Signup and view all the answers

There are how many equal energy p orbitals?

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

Hydrogen's principal energy level 1 consists of how many orbitals?

<p>1s</p> Signup and view all the answers

All p orbitals are shaped this way.

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

The arrangement of electrons in an atom's ___.

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

Electrons in an atom tend to assume the arrangement that gives the atom the ___ possible energy.

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

This arrangement of electrons is the most ___ arrangement and is the atom's ___.

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

What are the electrons in an atom's outermost orbitals called?

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

What principle states that each electron occupies the lowest energy orbital level available?

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

In an electron-dot structure, the element's symbol represents the...

<p>atom's nucleus and inner electrons</p> Signup and view all the answers

What are the valence electrons in Cl? [Ne]3s^2 3p^5

<p>5</p> Signup and view all the answers

Which electrons are represented by the dots in an electron-dot structure?

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

Flashcards

Electromagnetic Radiation

Energy traveling as waves through space, including light, x-rays, radio waves, and microwaves.

Wavelength

Shortest distance between equivalent points on a wave.

Amplitude

Height of a wave from origin to crest or trough.

Frequency

Number of waves per second, measured in Hertz (Hz).

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Quantum

Minimum energy atom can lose or gain.

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Photoelectric Effect

Electrons emitted from metal surface by light.

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Atomic Emission Spectrum

Unique set of colors/frequencies emitted by an element.

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Flame Test

Identifying elements by their unique colors in a flame.

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Bohr's Atomic Model

Model predicting hydrogen's emission spectrum; electrons orbit nucleus in specific energy levels.

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Quantum Mechanical Model

Model treating electrons as waves, based on Schrödinger's equation.

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Heisenberg Uncertainty Principle

Impossible to know both electron's position and velocity precisely.

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Atomic Orbital

Three-dimensional area around the nucleus where electron is likely to be.

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Electron Configuration

Arrangement of electrons in orbitals.

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S Orbital

Spherical electron orbital.

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P Orbital

Dumbbell-shaped electron orbital within the same energy level.

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Aufbau Principle

Electrons fill lowest energy orbitals first.

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Valence Electron

Outermost electrons influencing reactivity.

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Electron-dot structure

Shows nucleus and inner electrons, surrounded by dots showing valence electrons.

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Ground State

Lowest possible energy state for an atom.

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Study Notes

Electromagnetic Radiation

  • A form of energy that travels as a wave through space, can include light, x-rays, radio waves, and microwaves.
  • Waves can be characterized by four properties: wavelength, amplitude, frequency, and speed.

Key Wave Properties

  • Wavelength: The shortest distance between equivalent points on a wave.
  • Amplitude: The height of a wave from the origin to a crest or trough.
  • Frequency: Measured in hertz (Hz), equivalent to one wave per second.

Energy and Photons

  • Quantum: Minimum energy that can be lost or gained by an atom.
  • Energy can only be emitted or absorbed in whole-number multiples according to Planck’s theory.
  • The energy of a photon is calculated using the equation (E = hv), where (h) is Planck’s constant.

Atomic Emission

  • Photoelectric Effect: Electrons are emitted from a metal's surface when it is illuminated with light of certain frequencies.
  • Each element has a unique atomic emission spectrum.
  • A flame test can identify elements based on their atomic emission spectrum, which consists of specific colors and frequencies unique to each element.

Bohr's Atomic Model

  • Predicts frequencies of lines in hydrogen’s atomic emission spectrum.
  • Electrons occupy orbits around the nucleus, with lower orbits corresponding to lower energy levels.
  • Electrons can move to higher-energy orbits when energy is added and emit photons corresponding to energy level transitions.
  • Model fails for elements beyond hydrogen concerning atomic emission spectra.

Quantum Mechanical Model

  • Treats electrons as waves and is based on the Schrödinger wave equation.
  • Heisenberg Uncertainty Principle: It’s impossible to know both the velocity and position of an electron simultaneously.
  • Atomic Orbital: A three-dimensional region around the nucleus representing the probability of an electron's location.

Electron Configuration

  • Each orbital can hold a maximum of two electrons.
  • S Orbitals: Spherically shaped; there is one s orbital within the first principal energy level.
  • P Orbitals: Dumbbell-shaped; consist of three equal-energy orbitals.
  • Electrons arrange themselves in a way that minimizes energy, achieving the lowest possible energy state (ground state).

Valence Electrons and Structure

  • Valence electrons are the outermost electrons influencing chemical reactivity.
  • The Aufbau Principle states that electrons fill the lowest energy orbitals first.
  • Electron-dot structures represent an atom's nucleus and inner electrons with the elemental symbol, while dots indicate valence electrons.

Chlorine Valence Electrons

  • Chlorine has five valence electrons from its electron configuration ([Ne]3s^2 3p^5).

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Description

This study guide contains flashcards covering essential concepts from Chapter 5 on electrons in atoms. Learn about electromagnetic radiation, its characteristics, and types such as light, x-rays, and microwaves. Perfect for mastering the fundamental principles of atomic structure.

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