Atomic Structure Review for Chemistry

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Questions and Answers

What is the correct electron configuration for the element Magnesium (Mg)?

  • 1s2 2s2 2p6 3s2 (correct)
  • 1s2 2s2 3s2
  • 1s2 2s2 2p6 3s1
  • 1s2 2s2 2p6 4s2

Which element is represented by the electron configuration 1s2 2s2 2p6 3s2 3p64s23d104p3?

  • Arsenic (As) (correct)
  • Selenium (Se)
  • Germanium (Ge)
  • Gallium (Ga)

In orbital notation, how many electrons can the 'd' subshell accommodate?

  • 14
  • 10 (correct)
  • 5
  • 2

What configuration error occurs when two 'p' electrons share the same orbital while others remain empty?

<p>Hund's Rule is violated (B)</p> Signup and view all the answers

Which subshell must completely fill before any electrons occupy the 'p' subshell?

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

What determines the mass number of an atom?

<p>The sum of protons and neutrons (C)</p> Signup and view all the answers

Which particle has a negative charge?

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

In an electrically neutral atom, how do the number of protons compare to the number of electrons?

<p>Protons and electrons are equal (D)</p> Signup and view all the answers

What makes an atom an ion?

<p>It has a net electrical charge due to unequal protons and electrons (A)</p> Signup and view all the answers

How do isotopes of the same element differ?

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

Which isotope of silicon has the greatest representation by percentage?

<p>Si-28 (D)</p> Signup and view all the answers

What is the charge of an atom with 8 protons and 10 electrons?

<p>-2 (B)</p> Signup and view all the answers

What is the average atomic mass of silicon given its isotopes' percentages?

<p>28.09 (C)</p> Signup and view all the answers

Which isotope of potassium is the most abundant?

<p>K-39 (C)</p> Signup and view all the answers

What happens to frequency when wavelength increases?

<p>Frequency decreases (C)</p> Signup and view all the answers

Which transition emits light with the highest frequency?

<p>n=6 to n=2 (C)</p> Signup and view all the answers

How many total electrons can be held by the 4p sublevel?

<p>6 (A)</p> Signup and view all the answers

How does an electron move when it absorbs energy?

<p>From lower energy level to higher energy level (B)</p> Signup and view all the answers

Which electron transition will absorb light with the highest energy?

<p>n=6 to n=2 (D)</p> Signup and view all the answers

What is the maximum number of electrons in one orbital of the 5d sublevel?

<p>2 (C)</p> Signup and view all the answers

Which sublevels are available in the 3rd energy level?

<p>s, p, d (B)</p> Signup and view all the answers

Flashcards

Proton

The positively charged particle found in the nucleus of an atom.

Neutron

The neutrally charged particle found in the nucleus of an atom.

Electron

The negatively charged particle found orbiting the nucleus of an atom.

Mass Number

The total count of protons and neutrons in an atom's nucleus.

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Charge

The difference between the number of protons and electrons in an atom.

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Atomic Number

The unique number of protons in an atom's nucleus, defining the element.

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Isotopes

Atoms of the same element with the same number of protons but a different number of neutrons.

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Ion

An atom or molecule with a net electrical charge.

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Electron Configuration and Chemical Properties

Elements within a group on the periodic table share the same electron configuration in their outermost shell. This is why elements within a group have similar chemical properties due to their tendency to lose or gain electrons in similar ways.

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Periodic Table Blocks

The s-block encompasses group 1 and 2 elements, the p-block elements span groups 13 to 18, the d-block represents transition metals from group 3 to 12, and the f-block elements are the lanthanides and actinides.

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Orbital Notation

Orbital notation depicts the distribution of electrons within different orbitals, represented by arrows that symbolize electrons with opposite spins.

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Hund's Rule

The Hund's rule dictates that electrons occupy individual orbitals within a subshell before doubling up in any one orbital. This ensures that electrons are as spread out as possible, minimizing repulsion.

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Aufbau Principle

The Aufbau principle states that electrons fill orbitals in order of increasing energy levels. This principle guides the electron configuration of atoms.

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Abundant Isotopes and Average Atomic Mass

The average atomic mass of an element is calculated by taking into account the relative abundance of each isotope. For example, if potassium-39 is the most abundant isotope of potassium, it will contribute the most to the overall average atomic mass of potassium.

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Wavelength and Frequency

The frequency of light is inversely proportional to its wavelength. This means that as the wavelength increases, the frequency decreases, and vice-versa.

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Energy and Frequency

The energy of light is directly proportional to its frequency. Higher frequency light carries more energy.

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Electron Transition: Emission

An electron moves from a higher energy level to a lower energy level when it releases energy, often in the form of light. This is known as an emission process.

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Electron Transition: Absorption

An electron moves from a lower energy level to a higher energy level when it absorbs energy, often in the form of light. This is known as an absorption process.

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Highest Frequency Emission

Electron transitions that result in the emission of light with the highest frequency correspond to the largest energy difference between the initial and final energy levels.

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Highest Energy Absorption

Electron transitions that result in the absorption of light with the highest energy correspond to the largest energy difference between the initial and final energy levels.

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Electron Capacity of an Orbital

Each orbital within a sublevel can hold a maximum of two electrons, with opposite spins.

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Study Notes

Atomic Structure Review

  • Subatomic Particles:
  • Protons: Small mass, positive charge, located in the nucleus.
  • Neutrons: Small mass, neutral charge, located in the nucleus.
  • Electrons: Small mass, negative charge, located in energy levels surrounding the nucleus.

Determining Atomic Properties

  • Mass Number: Sum of protons and neutrons.
  • Charge: Difference between the number of protons and electrons.
  • Atomic Number: Number of protons in an atom.

Atomic Structure Sketch

  • A sketch of an atom with 3 protons, 4 neutrons, and 2 electrons should be drawn, showing the nucleus with the protons and neutrons, and the electron cloud surrounding the nucleus.

Atomic Table Completion

  • The table provides information about various elements including their symbol, atomic number, mass number, charge, proton count, neutron count, and electron count.
  • Examples: Magnesium-24 has 12 protons, 12 neutrons, and 12 electrons .
  • Oxygen-16 has 8 protons, 8 neutrons, and 8 electrons

Ions Identification

  • Ions are atoms or molecules with a net electric charge.
  • Elements in the table with a charge indicating a difference between protons and electrons are ions
  • Examples: Oxygen (O-16) and Sodium (Na).

Isotopes

  • Isotopes are atoms of the same element with different numbers of neutrons.
  • They share the same number of protons but differ in mass number.
  • Examples: Silicon-28, Silicon-29, and Silicon-30 are isotopes of silicon.

Average Atomic Mass Calculation

  • The average atomic mass of an element is calculated by considering the abundance of each isotope.
  • Examples: Determine the average atomic mass of silicon given the percentage amounts and mass of each isotope.

Determining the Most Abundant Isotope

  • An element's most abundant isotope will be the isotope that contributes most to the element's average atomic mass. (based on percentage abundance.

Relationship Between Wavelength and Frequency

  • Wavelength and frequency are inversely related.
  • As one increases, the other decreases.

Relationship Between Energy and Frequency

  • Energy and frequency are directly related.
  • As one increases, the other increases.

Emission Spectra and Energy Levels

  • Electrons absorb energy and move to higher energy levels.
  • Electrons release energy and move to lower energy levels.
  • This energy change is often emitted as light with specific wavelengths (colors).

Determining Electron Transitions

  • Electron transitions between energy levels determine the energy and frequency of emitted light.
  • Higher frequency transitions involve higher energy differences.

Electron Configuration

  • Electron configurations describe how electrons are arranged in atoms. Sublevels within energy levels.
  • Sublevels (s,p,d,f) have orbitals that relate to electron numbers and the order filling.
  • Rules apply (e.g. Aufbau principle, Hund's rule)

Orbital Notation

  • Orbital notations visualize electron distribution in atomic orbitals.

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