Atomic Models, Energy & Electrons

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Questions and Answers

Consider two isotopes of the same element. Which statement accurately describes the relationship between them?

  • They have the same number of neutrons but a different number of protons.
  • They have the same number of protons but a different number of neutrons. (correct)
  • They have the same number of protons but a different number of electrons.
  • They have the same mass number but a different atomic number.

In Rutherford's gold foil experiment, what observation led him to conclude that the atom is mostly empty space with a small, dense, positively charged nucleus?

  • All alpha particles passed straight through the gold foil.
  • Most alpha particles were deflected at large angles.
  • Most alpha particles passed straight through the gold foil with little to no deflection. (correct)
  • Alpha particles were absorbed by the gold foil.

According to Bohr's model, what determines the energy of an electron in an atom?

  • The shape of the electron's orbit.
  • The speed at which the electron is moving.
  • The number of protons in the nucleus.
  • The specific orbit or energy level the electron occupies. (correct)

How does the quantum mechanical model describe the location of electrons in an atom, and how does this differ from Bohr's model?

<p>The quantum model describes electrons in probability clouds or orbitals, while Bohr's model describes them in fixed paths. (B)</p>
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An electron transitions from a higher energy level to a lower energy level in an atom. What is the consequence of this transition?

<p>The atom emits energy in the form of electromagnetic radiation. (C)</p>
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Which of the following best explains the relationship between the energy of a photon and its frequency?

<p>The energy of a photon is directly proportional to its frequency. (D)</p>
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Given the electron configuration of an element is $1s^22s^22p^63s^23p^5$, how many valence electrons does this element have, and to which group does it belong?

<p>7 valence electrons, Group 17 (B)</p>
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According to the Heisenberg uncertainty principle, what is the fundamental limitation on our knowledge of an electron's properties?

<p>We cannot simultaneously know both the exact position and momentum of an electron. (A)</p>
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Which of the following describes the shape and spatial orientation of the p orbitals in an atom?

<p>Dumbbell shape, with three orbitals oriented mutually perpendicular along the x, y, and z axes. (D)</p>
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How does the Aufbau principle guide the filling of electron orbitals in an atom, and what is its significance?

<p>Electrons first fill the orbitals with the lowest energy levels, which determines the electron configuration. (B)</p>
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If an element is in the d-block of the periodic table, what can you infer about its electron configuration?

<p>Its outermost electrons are filling d orbitals. (C)</p>
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What is the significance of valence electrons in determining the chemical properties of an element?

<p>Valence electrons participate in chemical bonding and determine an element's reactivity. (D)</p>
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How does ionization energy generally change as you move across a period from left to right on the periodic table, and what causes this trend?

<p>It increases due to increasing nuclear charge and decreasing atomic radius. (A)</p>
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Which of the following best describes the trend in atomic radius as you move down a group on the periodic table, and what is the primary reason for this trend?

<p>Atomic radius increases because additional electron shells are added. (C)</p>
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What is electronegativity, and how does it influence the type of chemical bond that forms between two atoms?

<p>Electronegativity is the ability of an atom to attract electrons in a chemical bond; a large difference leads to ionic bonds, while a small difference leads to covalent bonds. (D)</p>
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How do metals typically achieve a stable electron configuration when forming ions, and what type of ion do they become?

<p>Metals lose electrons to achieve a full outer shell, forming cations. (A)</p>
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Describe the formation of an ionic bond between sodium (Na) and chlorine (Cl), and explain why this bond is formed.

<p>Sodium transfers an electron to chlorine, forming $Na^+$ and $Cl^-$ ions, which are attracted to each other due to opposite charges. (C)</p>
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What properties are characteristic of ionic compounds, and how do these properties relate to the nature of ionic bonding?

<p>High melting points, brittleness, and electrical conductivity when dissolved in water; these properties result from strong electrostatic forces between ions. (D)</p>
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Consider the compound magnesium oxide (MgO). How would you name this compound following the rules of ionic nomenclature?

<p>Magnesium oxide (C)</p>
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A neutral atom has the following electron configuration: $1s^22s^22p^63s^23p^64s^1$. What ion is this atom most likely to form, and what will be its charge?

<p>It will lose one electron to form a cation with a +1 charge. (A)</p>
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Flashcards

Dalton's Atomic Model

Atoms are tiny, solid, indivisible spheres.

Thomson's Atomic Model

Discovered electrons, proposed the "plum pudding" model.

Rutherford's Gold Foil Experiment

Atoms are mostly empty space with a small, dense, positive nucleus.

Bohr's Atomic Model

Electrons orbit the nucleus in fixed energy levels or orbits.

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Quantum Model of the Atom

Electrons exist in probability clouds (orbitals), not fixed paths.

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Ground State

The state where an electron occupies the lowest available energy level.

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Excited State

The state where an electron has absorbed energy and moved to a higher energy level.

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Electron Capacity of Orbitals

Each orbital holds a maximum number of electrons: s=2, p=6, d=10, f=14.

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Heisenberg Uncertainty Principle

It is impossible to know both the position and momentum of an electron with perfect accuracy.

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Wavelength and Frequency Relationship

Shorter wavelengths correspond to higher frequency and higher energy.

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Visible Light Spectrum (ROYGBIV)

Visible light colors ordered from lowest to highest energy: Red, Orange, Yellow, Green, Blue, Indigo, Violet.

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Alkali Metals

Highly reactive metals with one valence electron in their outermost shell.

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Halogens

Highly reactive nonmetals that need to gain one electron to have a full outer shell.

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Noble Gases

Elements with full outer electron shells, making them very stable and unreactive.

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Atomic Radius Trend (Across Period)

Decreases from left to right across a period due to increasing nuclear charge.

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Ionization Energy Trend (Down a Group)

Energy decreases as you go down a group because the outermost electrons are farther from the nucleus.

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Cation

A positively charged ion formed when an atom loses electrons.

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Anion

A negatively charged ion formed when an atom gains electrons.

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Ion Formation

Metals lose electrons to form positive ions; nonmetals gain electrons to form negative ions.

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Properties of Ionic Compounds

High melting points, brittle, and conduct electricity when dissolved in water.

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Study Notes

Atomic Models & Theory

  • Dalton proposed that atoms are indivisible, tiny, solid spheres.
  • Thomson's "plum pudding" model led to the discovery of electrons.
  • Rutherford's gold foil experiment revealed that atoms are mostly empty space.
  • Bohr described electrons moving in fixed orbits or levels around the nucleus.
  • The quantum model describes electrons existing in clouds, not fixed paths.

Energy & Electrons

  • An electron jumps to a higher energy level when it absorbs energy.
  • An excited electron releases light when it falls back to its ground state.
  • The ground state has less energy than the excited state.
  • More energy corresponds to an electron being farther from the nucleus.

Electron Configuration & Quantum Numbers

  • The order of orbitals for electron configuration is 1s 2s 2p 3s 3p 4s 3d.
  • The s orbital can hold 2 electrons, the p orbital can hold 6, the d orbital can hold 10, and the f orbital can hold 14.
  • The s orbital has a spherical shape.
  • The p orbitals have a dumbbell shape.
  • The d-block on the periodic table can hold 10 electrons.
  • Heisenberg's uncertainty principle states that one cannot simultaneously know both the speed and position of an electron.
  • Higher frequency light has more energy.
  • Shorter wavelength means higher frequency.
  • Violet light has the most energy among the colors of visible light.
  • The visible light colors, ordered from lowest to highest energy, are Red, Orange, Yellow, Green, Blue, Indigo, Violet (ROYGBIV).

Periodic Table & Trends

  • Alkali metals have 1 valence electron and are very reactive.
  • Halogens are highly reactive because they need to gain 1 electron to achieve a full outer shell.
  • Noble gases do not typically form bonds because they have full outer shells.
  • Atomic radius decreases from left to right across a period.
  • Ionization energy decreases as you move down a group.
  • Electronegativity increases up and to the right on the periodic table.

Ions & Ionic Bonding

  • A cation is a positive ion, and an anion is a negative ion.
  • A metal becomes a cation by losing electrons.
  • Nonmetals form anions.
  • An ionic compound like NaCl is named sodium chloride.
  • Ionic compounds are typically brittle, have high melting points, and conduct electricity when dissolved in water.

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