Electron Chemistry and Atomic Theory
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Questions and Answers

What is indicated by the number at the top of an element in the periodic table?

  • Atomic number (correct)
  • Mass number
  • Valence electrons
  • Period number

Which group in the periodic table contains elements that have two valence electrons?

  • Group 7
  • Group 1
  • Group 2 (correct)
  • Group 8

What do all elements in the same group of the periodic table share in common?

  • Same mass number
  • Same number of occupied shells
  • Same atomic number
  • Same number of valence electrons (correct)

What is the primary reason most elements form compounds?

<p>To obtain a full outer shell of electrons (B)</p> Signup and view all the answers

What type of bond involves the electrostatic attraction between ions of opposite charge?

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

Which of the following statements best describes the valence electrons of elements in group 7?

<p>They have seven valence electrons. (C)</p> Signup and view all the answers

What determines the period number of an element in the periodic table?

<p>The number of occupied electron shells (C)</p> Signup and view all the answers

In Bohr's theory, what does the energy level of an element correspond to?

<p>The element's position in the periodic table (D)</p> Signup and view all the answers

What happens to white light when it passes through a hydrogen gas flask?

<p>The light disperses into colors with black lines at certain wavelengths. (A)</p> Signup and view all the answers

What is the highest energy level for an argon atom based on its electron configuration?

<p>3 (D)</p> Signup and view all the answers

In Bohr's theory, how many electrons can the first shell hold?

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

Which of the following describes the nature of electrons in relation to energy levels?

<p>Electrons can only exist within specific orbitals that have fixed energies. (C)</p> Signup and view all the answers

What characterizes the arrangement of elements in the periodic table?

<p>Elements are arranged by their atomic number. (D)</p> Signup and view all the answers

How many electrons can the second shell hold according to Bohr's theory?

<p>8 (A)</p> Signup and view all the answers

Which statement is true regarding the movement of electrons between energy levels?

<p>Electrons require a specific quantum of energy to move up or down energy levels. (C)</p> Signup and view all the answers

Based on the rules for electron configuration, which of the following configurations is correct for magnesium?

<p>2, 8, 2 (B)</p> Signup and view all the answers

What occurs when two pairs of electrons are shared between two atoms?

<p>A double covalent bond is formed. (A)</p> Signup and view all the answers

What characteristic of polar molecules affects their interaction with non-polar molecules?

<p>They are hydrophilic. (C)</p> Signup and view all the answers

What phenomenon causes hydrogen bonding in water?

<p>Attractive forces between hydrogen and electronegative elements. (B)</p> Signup and view all the answers

How does electronegativity influence the distribution of electrons in a covalent bond?

<p>Electrons tend to be shifted toward the more electronegative atom. (A)</p> Signup and view all the answers

What is a characteristic feature of compounds with a hydrogen bond?

<p>They demonstrate strong dipole-dipole attractions. (D)</p> Signup and view all the answers

Which type of molecule is referred to as hydrophobic?

<p>Molecules that dissolve in fats and oils. (D)</p> Signup and view all the answers

What type of bond is formed when three pairs of electrons are shared between two atoms?

<p>A triple covalent bond. (A)</p> Signup and view all the answers

What effect does the constant motion of electrons in an atom or molecule create?

<p>Oscillating electron dipoles. (B)</p> Signup and view all the answers

Flashcards

Electron Orbitals

Specific regions around an atom's nucleus where electrons can exist.

Energy Levels

The fixed energies associated with electron orbitals.

Quantum of Energy

The exact amount of energy needed to move an electron between energy levels.

Bohr's Theory

A model describing electron arrangement in atoms, stating that electrons exist in specific energy levels.

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Electron Configuration

The arrangement of electrons in the energy levels of an atom.

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Energy Level Filling

Electrons will first occupy the lowest energy levels first.

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Electron Shell Capacity

The maximum number of electrons that can fit into each electron shell.

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Periodic Table

A tabular arrangement of elements based on atomic number.

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Atomic Number

The number of protons in an atom's nucleus, unique to each element.

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Mass Number

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

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Valence Electrons

Electrons in the outermost energy level of an atom.

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Groups (Periodic Table)

Vertical columns of elements on the periodic table; elements in a group have the same number of valence electrons.

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Periods (Periodic Table)

Horizontal rows of elements on the periodic table; elements in a period have the same number of occupied electron shells.

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Alkali Metals

Group 1 elements, very reactive, have one valence electron.

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Ionic Bond

Electrostatic attraction between oppositely charged ions.

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Full Outer Shell

The most stable electron configuration for an atom, achieved through bonding.

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Double covalent bond

Two pairs of electrons shared between two atoms.

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Triple covalent bond

Three pairs of electrons shared between two atoms.

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Electronegativity

Atom's tendency to attract bonding electrons.

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Dipole-dipole attraction

Electrostatic attraction between polar molecules.

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Hydrogen bond

Strong dipole-dipole attraction between molecules with H and highly electronegative atoms(O).

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Polar molecule

Molecule with uneven electron distribution, creating partial charges.

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Hydrophilic

Polar molecules that dissolve in water.

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Hydrophobic/Lipophilic

Non-polar molecules that do not dissolve in water, but dissolve in fats and oils.

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Study Notes

Electron Chemistry

  • White light dispersed by prism into component colours
  • Passing white light through hydrogen gas produces black lines at specific wavelengths
  • Atoms have nucleus surrounded by energy levels/orbitals where electrons exist
  • Electrons can only exist within specific orbitals
  • Electrons need fixed energy amounts to move between orbitals
  • This fixed energy amount is called a quantum/photon
  • Energy levels are represented by straight lines, not orbitals as 'planets around the sun'
  • The lowest energy level, n=1, is closest to the nucleus

Bohr's Theory

  • Electrons occupy the lowest possible energy levels
  • First shell holds up to 2 electrons
  • Second shell holds up to 8 electrons
  • Third shell (and subsequent shells) hold up to 8 electrons

Atomic Configurations

  • Example: Argon (atomic number 18) has electronic configuration 2, 8, 8
  • Example: Magnesium (atomic number 12) has electronic configuration 2, 8, 2

The Periodic Table

  • Tabular arrangement of chemical elements according to atomic number
  • Atomic number at top of box
  • Mass number at bottom of box
  • Elements classified as metals, metalloids, or nonmetals
  • Elements in groups have the same number of valence electrons
  • Valence electrons: same as group number

Group 1 Elements (Alkali Metals)

  • Have one valence electron
  • Very reactive
  • Form compounds in consistent ratios

Group 2 Elements (Alkaline Earth Metals)

  • Have two valence electrons
  • Less reactive than Group 1 elements

Group 7 Elements (Halogens)

  • Have seven valence electrons
  • Reactive, readily gain electrons

Group 8 Elements (Noble Gases)

  • Have eight valence electrons
  • Relatively unreactive

Periods

  • Horizontal rows in the periodic table
  • Period number corresponds to number of occupied electron shells

Bonding

  • Elements bond to achieve full outer electron shells
  • Ionic bond: electrostatic attraction between oppositely charged ions (metal + nonmetal)
    • Example: sodium (Na) and chlorine (Cl) form sodium chloride (NaCl). Sodium loses an electron, becomes positive ion; chlorine gains electron, becomes negative ion
  • Covalent bond: sharing of electron pairs (nonmetal + nonmetal)
    • Single, double, or triple covalent bonds depending on shared electron pairs
  • Dipole-Dipole attractions: unequal sharing of electrons in covalent bonds creates partial charges, leading to attractions between molecules
  • Hydrogen bonding: a strong dipole-dipole attraction involving hydrogen and a highly electronegative atom (e.g., oxygen)
  • Van der Waals' Forces: weak attractive forces caused by temporary fluctuations in electron distribution around atoms or molecules

Metallic Bonding

  • Consists of an array of cations in a "sea of delocalised electrons"
  • Good electrical and thermal conductors because electrons can freely move throughout the structure

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Electron Chemistry PDF

Description

Test your knowledge of electron chemistry, Bohr's theory, and atomic configurations. This quiz covers fundamental concepts including the structure of atoms, energy levels, and the periodic table. Dive into the intricacies of how electrons are arranged around the nucleus and their energy transitions.

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