Atomic Structure and Subatomic Particles
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Questions and Answers

How many neutrons are there in a lithium atom with a mass number of 7 and an atomic number of 3?

  • 4 (correct)
  • 2
  • 3
  • 5

What is the maximum number of electrons that can occupy the second orbit according to Bohr's model?

  • 2
  • 8 (correct)
  • 18
  • 6

Which quantum number indicates the main energy level occupied by an electron?

  • Angular momentum quantum number
  • Principal quantum number (correct)
  • Spin quantum number
  • Magnetic quantum number

In the electron cloud model, what does the 'cloud' represent?

<p>The region where electrons are likely to be found (B)</p> Signup and view all the answers

What is the maximum number of electrons the third orbit can hold?

<p>18 (A)</p> Signup and view all the answers

Which type of quantum number indicates the shape or type of orbital occupied by an electron?

<p>Angular momentum quantum number (C)</p> Signup and view all the answers

How is the mass of an atom described in Bohr's model?

<p>Concentrated at the nucleus (C)</p> Signup and view all the answers

What do the values of the principal quantum number (n) represent?

<p>The main energy level of the electron (A)</p> Signup and view all the answers

Which subatomic particle is negatively charged?

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

What is the atomic number of an element defined as?

<p>The number of protons in an atom (D)</p> Signup and view all the answers

How do isotopes of an element differ from each other?

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

Which of the following statements is true regarding atomic structure?

<p>Atoms are always neutral due to equal protons and electrons. (A)</p> Signup and view all the answers

What is the mass number of an atom with 15 protons and 10 neutrons?

<p>25 (D)</p> Signup and view all the answers

Which of the following particles has the greatest mass?

<p>Both neutron and proton (B)</p> Signup and view all the answers

If an atom contains 12 protons, what is its atomic number?

<p>12 (D)</p> Signup and view all the answers

What determines the identity of an atom?

<p>The number of protons (D)</p> Signup and view all the answers

What is the maximum number of electrons that can occupy the second energy level?

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

Which principle states that no two electrons in the same orbital can have the same spin?

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

Which sublevel can contain a maximum of 10 electrons?

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

For an orbital with an angular momentum quantum number (L) of 1, which type of orbital is it?

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

Which of the following statements is consistent with Hund's Rule?

<p>Electrons will occupy separate orbitals of the same energy before pairing. (C)</p> Signup and view all the answers

An atom with 6 protons and 8 neutrons is classified as which of the following?

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

Which understanding is essential to following the Aufbau Principle?

<p>Orbitals fill in order of increasing energy. (B)</p> Signup and view all the answers

Which orbital can hold a maximum of 14 electrons?

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

Flashcards

What is an atom?

A basic unit of matter. Everything is made up of atoms.

What are subatomic particles?

Smaller particles that make up an atom.

What is an electron?

A negatively charged subatomic particle that orbits the nucleus of an atom.

What is a proton?

A positively charged subatomic particle located in the nucleus of an atom. The number of protons determines the element.

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What is a neutron?

A neutral subatomic particle located in the nucleus of an atom. It has no charge.

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What is the atomic number?

The number of protons in an atom's nucleus. It identifies the element.

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What is the mass number?

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

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What are isotopes?

Atoms of the same element that have the same number of protons but a different number of neutrons. They have the same atomic number but different mass numbers.

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Atomic Number

The number of protons in an atom's nucleus, determining its chemical identity.

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Mass Number

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

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Calculating Number of Neutrons

The number of neutrons can be calculated by subtracting the atomic number from the mass number. (Number of neutrons = Mass number - Atomic number)

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Nucleus

The positively charged center of an atom containing protons and neutrons.

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Electrons

Negatively charged particles that orbit the nucleus in specific energy levels.

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Atomic Structure

Describes the arrangement of electrons around the nucleus in specific energy levels or shells.

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Bohr's Model

A model that depicts electrons orbiting the nucleus in distinct circular paths or energy levels.

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Electron Cloud Model

A probability model that describes the likelihood of finding an electron within a specific region of space around the nucleus.

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Main Energy Level (n)

The main energy level of an atom, represented by the principal quantum number (n). It describes the electron's average distance from the nucleus. Higher values of 'n' indicate higher energy levels and greater distance from the nucleus.

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Sublevels (L)

The shape of an electron's orbital, determined by the angular momentum quantum number (L). Each value of 'L' represents a different sublevel: s (L=0), p (L=1), d (L=2), f (L=3).

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Orbital Orientation (m)

The orientation of an electron's orbital in space, determined by the magnetic quantum number (m). Each sublevel has multiple orbitals, each oriented differently.

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Electron Spin (s)

The intrinsic angular momentum of an electron, represented by the spin quantum number (s). Electrons spin like tiny magnets, either clockwise (+1/2) or counterclockwise (-1/2).

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Aufbau Principle

The principle that states that orbitals are filled in order of increasing energy, starting with the lowest energy level and moving up.

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Pauli Exclusion Principle

The principle that states that only two electrons can occupy an orbital, and their spins must be opposite (paired).

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Hund's Rule

The rule that states that for orbitals with equal energy (degenerate orbitals), electrons will fill each orbital individually before pairing up in any one orbital.

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Electron Configuration

The arrangement of electrons in the different energy levels and sublevels of an atom, represented by a notation that indicates the number of electrons in each orbital.

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Study Notes

Atom Structure

  • Atoms are the fundamental building blocks of matter
  • Matter is anything that occupies space and has mass
  • Understanding atomic structure is crucial to understanding the properties of matter

Subatomic Particles

  • Subatomic particles make up atoms
  • Key subatomic particles for chemistry are electrons, protons, and neutrons
  • Electrons have a negative charge
  • Protons have a positive charge
  • Neutrons have no charge

Properties of Subatomic Particles

  • | Name | Symbol | Charge | Common charge | Mass (kg) |
  • |---|---|---|---|---|
  • | Electron | e, e-, or -10e| -1 | -1.602 × 10⁻¹⁹ | 9.109 × 10⁻³¹ |
  • | Proton | p, p+, or ₁P | +1 | +1.602 × 10⁻¹⁹ | 1.673 × 10⁻²⁷ |
  • | Neutron | n or °₁n | 0 | 0 | 1.675 × 10⁻²⁷ |

Atoms and Neutrons

  • Number of protons equals the number of electrons in a neutral atom
  • Neutrons do not affect the overall charge of the atom

Atomic Number

  • Atomic number indicates the number of protons in an atom
  • The number of protons defines the type of atom

Mass Number

  • Mass number is the sum of protons and neutrons in an atom's nucleus
  • Mass number - Atomic number = Number of neutrons

Determining Subatomic Particles

  • Using the provided table, students can determine the number of protons, neutrons, and electrons for different elements

Bohr's Model

  • Atom has a positively charged central part called the nucleus
  • Nucleus contains protons and neutrons
  • Electrons orbit the nucleus at specific energy levels (fixed distances from the nucleus).
  • Each electron orbit holds a maximum number of electrons – ( 2n² ) whereby n is the orbit level.

Electron Cloud Model

  • This is a probability model
  • Electrons are located in orbitals (regions of space) where they are likely to be found
  • Position of electrons is based on mathematical equations

Quantum Numbers

  • Four quantum numbers define the region where electrons reside:
  • Principal quantum number (n) : Energy level of the electron
  • Angular momentum quantum number (L) : Shape and type of orbital
  • Magnetic quantum number (m) : Orbitals number and orientations
  • Spin (s) : Intrinsic angular momentum
  • Values of sublevels (s, p, d, f...) are assigned. 0, 1, 2, 3 correspond to s, p, d, f respectively.
  • The table shows the quantum numbers of the first 30 atomic orbitals

Electron Configuration

  • Arrangement of electrons in an atom
  • Each energy level can hold a specific maximum number of electrons (2n²)
  • Energy levels are further divided into sublevels called orbitals, designated by letters (s, p, d, f...)

Electron Configuration Principles

  • Aufbau Principle: Electrons fill orbitals from lowest energy to highest energy
  • Pauli Exclusion Principle: Each orbital can hold a maximum of two electrons with opposite spins
  • Hund's Rule: When orbitals of equal energy are available, electrons first occupy each orbital singly with parallel spins before pairing up

Isotopes

  • Isotopes have the same number of protons (same atomic number) but different numbers of neutrons (different mass number)

Elements

  • An element is a substance composed of a single type of atom
  • There are about 90 naturally occurring elements, plus some lab-created ones

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Atomic Structure - 2 - PDF

Description

This quiz delves into the fundamental building blocks of matter, focusing on atomic structure and the characteristics of subatomic particles such as electrons, protons, and neutrons. Understanding these concepts is essential for grasping the properties of matter and the basics of chemistry.

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