Questions and Answers
What is the atomic number of an atom defined as?
Which particles are primarily located in the nucleus of an atom?
What are protons and neutrons collectively referred to as?
What are quarks and gluons primarily responsible for?
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Which subatomic particle is considered unstable and was discovered by James Chadwick?
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What is the location of protons within an atom?
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Which scientist is credited with the discovery of electrons?
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How do you determine the maximum number of electrons in a shell?
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According to the octet rule, how many electrons can the outermost shell hold?
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What is the relationship between protons and electrons in a stable atom?
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Study Notes
Atomic Structure Basics
- Atoms consist of two primary parts: the nucleus (centrally located) and orbital shells (outside the nucleus).
- Atomic number represents the number of protons in an atom.
- Atomic mass is the mass of a particle relative to the atom.
Subatomic Particles
- Three main constituents of an atom: electrons, protons, and neutrons.
- Protons and neutrons, located in the nucleus, are collectively called nucleons.
- Electrons are classified as leptons and are located in orbital shells.
Protons
- Serve as the identity of an atom; discovered by Ernest Rutherford.
- Each proton carries a positive charge; identified by Eugene Goldstein.
- Protons and neutrons are composed of quarks held together by gluons.
Neutrons
- Neutrons are considered unstable and were discovered by James Chadwick.
- Neutral charge indicates no net electrical charge; located in the nucleus.
Electrons
- Electrons are the lightest subatomic particles, approximately 2000 times lighter than protons and neutrons.
- They occupy orbital shells or extranuclear regions around the nucleus.
- In a stable atom, the number of electrons equals the number of protons.
Electron Configuration
- Electron arrangement follows Niels Bohr's systematic pattern.
- The outermost shell (valence shell) can hold up to eight electrons, following the OCTET Rule.
- Exception: K-shell can only accommodate two electrons.
Electron Binding Energy (EBE)
- EBE measures the strength of attachment between electrons and the nucleus.
- Closer electrons have higher EBE, resulting in stronger attractive forces.
- Greater atom size correlates with larger EBE and increased difficulty in ionization.
Ionization
- Ionization occurs when electrons are removed or added to an atom.
- The energy required for ionization must match or exceed the EBE.
- An atom becomes an ion when it gains or loses electrons.
Nuclear Families
- Isotopes: Atoms with the same number of protons but different neutrons.
- Isobars: Atoms with the same nucleon number.
- Isotones: Atoms with an identical number of neutrons.
- Isomers: Atoms with the same number of protons and neutrons but existing in different energy states.
Important Terms
- Matter: Anything that occupies space and possesses mass.
- Energy: Lacks occupied space, mass, or charge; transforms forms without creation or destruction.
- Mass: Basic particle of a compound, combining multiple atoms.
- Compound: A quantity of one type of molecule.
- Element: A pure substance composed of identical atoms.
Bonding
- Covalent Bonds: Involve sharing of electrons to create molecules.
- Ionic Bonds: Formed through attraction between ions with opposite charges.
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Description
Test your knowledge on the basic components of atomic structures. This quiz covers essential concepts like atomic number, atomic mass, and the roles of the nucleus and orbital shells. Perfect for students learning about the fundamentals of chemistry.
