Atomic Structure and Subatomic Particles
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Questions and Answers

What is the layout of an element?

mass # & atomic #

What is the atomic number?

of protons

What does the mass number equal?

of protons + neutrons

In a neutral atom, what does the number of protons equal?

<h1>of electrons</h1> Signup and view all the answers

How do you find the correct number of neutrons?

<p>mass number - atomic number</p> Signup and view all the answers

What are forms of the same elements that differ in the amount of neutrons?

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

What particle, if lost from the nucleus, would NOT cause a change in the atomic number?

<p>a neutron because it has no charge</p> Signup and view all the answers

What did Rutherford's experiment with alpha particles suggest?

<p>that the atoms of the metal were mostly empty space</p> Signup and view all the answers

To which group of elements on the periodic table does an atom with a valence shell configuration of 1s1 belong?

<p>IA alkali metals</p> Signup and view all the answers

What happens to the frequency of a photon when its wavelength increases?

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

What happens to the wavelength of a photon when its frequency increases?

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

What does C represent in the light energy formula?

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

What is the ground-state electron configuration of an atom in the second period?

<p>1s2 2s1</p> Signup and view all the answers

What is Hund's rule?

<p>Electrons do not pair until they have to.</p> Signup and view all the answers

What is paramagnetism?

<p>An experimental phenomena associated with atoms having unpaired electrons.</p> Signup and view all the answers

Which drop in energy level results in the greatest emission of energy?

<p>n=2 to n=1</p> Signup and view all the answers

What do the four quantum numbers stand for?

<p>n = energy level, l = (n-1), ml = -l to l, ms = 1/2 or -1/2 (spin)</p> Signup and view all the answers

What particles make up an alpha particle?

<p>2 protons and 2 neutrons</p> Signup and view all the answers

What did Millikan discover from his oil drop experiments?

<p>the magnitude of the charge on an electron</p> Signup and view all the answers

When an atom of an electropositive atom becomes an ion, what happens?

<p>it becomes larger</p> Signup and view all the answers

Nearly all the mass in an atom is located where?

<p>inside the nucleus</p> Signup and view all the answers

Classify the following as an element, compound, or mixture. If it is a mixture, decide if it is a homogeneous or heterogeneous mixture:

<p>Sugar = compound, not a mixture Spaghetti Sauce = mixture, heterogeneous Phosphorus = element</p> Signup and view all the answers

What are properties that depend on the amount of matter present called?

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

What are allotropes?

<p>two or more different physical forms in which an element can exist</p> Signup and view all the answers

What two subatomic particles have the most mass but occupy very little of the volume of an atom?

<p>protons and neutrons</p> Signup and view all the answers

Define isoelectronic.

<p>Having the same amount of electrons</p> Signup and view all the answers

How does a sodium ion differ from a sodium atom?

<p>the sodium ion has fewer electrons</p> Signup and view all the answers

What is the shape, electron domain geometry, and prefix for the Dz^2 orbital?

<p>information not provided</p> Signup and view all the answers

What does the Dxy orbital represent?

<p>information not provided</p> Signup and view all the answers

What does the Dx^2y^2 orbital represent?

<p>information not provided</p> Signup and view all the answers

Study Notes

Atomic Structure and Composition

  • Mass number equals the sum of protons and neutrons.
  • Atomic number indicates the number of protons in an atom and determines the element's identity.
  • A neutral atom has an equal number of protons and electrons.
  • Neutrons can be calculated by subtracting the atomic number from the mass number.
  • Isotopes are variations of the same element with differing neutron counts.

Atomic and Subatomic Particles

  • A neutron's removal from the nucleus does not alter the atomic number since it carries no charge.
  • Protons and neutrons comprise the majority of an atom's mass, located within the nucleus.

Electron Configuration

  • Atoms with a valence shell configuration of 1s1 belong to Group IA (alkali metals).
  • Ground-state electron configuration in the second period can be represented as 1s2 2s1.
  • Hund's rule states electrons will fill separate orbitals before pairing occurs.

Quantum Mechanics

  • Quantum numbers define an electron's state:
    • n (energy level),
    • l (orbital type),
    • ml (magnetic quantum number),
    • ms (spin).
  • The quantum numbers for each orbital are:
    • s: 1, 0, 0
    • p: 2, 1, -1, 0, 1
    • d: 3, 2, -2, -1, 0, 1, 2
    • f: 4, 3, -3, -2, -1, 0, 1, 2, 3.

Electromagnetic Radiation

  • The electromagnetic spectrum is characterized by photons, where an increase in wavelength corresponds to a decrease in frequency, and vice versa.

Atomic Mass and Charge

  • An alpha particle consists of 2 protons and 2 neutrons; they represent a significant mass but occupy a negligible atomic volume.
  • Millikan's experiments determined the charge value of an electron.

Chemical Concepts

  • Compounds have fixed ratios of different elements, while mixtures do not; mixtures can be homogeneous or heterogeneous.
  • Isomers are compounds with the same molecular formula but distinct structural arrangements and properties.
  • Allotropes refer to different structural forms of the same element; for example, carbon can exist as graphite, charcoal, or diamond.

Ions and Electron Count

  • A sodium ion has fewer electrons than a neutral sodium atom, leading to an overall positive charge.
  • When a neutral electropositive atom becomes an ion, its radius generally increases.

Properties of Matter

  • Extensive properties depend on the amount of substance present; examples include mass and volume.
  • Distinction between elements (pure substances), compounds (substances made of two or more elements), and mixtures is crucial in chemistry.

General Observations

  • Rutherford's gold foil experiment suggested that atoms are mostly empty space with a dense nucleus containing positively charged particles.
  • Paramagnetism is observed in atoms having unpaired electrons, causing attraction to magnetic fields.

Orbital Types

  • Specific types of orbitals such as dz², dxy, and dx²y² define the shape and type of electron domains within an atom, impacting chemical bonding and properties.

These notes provide a clear overview of fundamental concepts crucial for understanding atomic structure, electron configuration, quantum mechanics, and chemical properties.

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Description

This quiz covers the essential concepts of atomic structure, including mass number, atomic number, and electron configuration. Test your understanding of atomic and subatomic particles, isotopes, and principles of quantum mechanics. Perfect for students studying chemistry or physics!

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