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Questions and Answers
Which subatomic particle has a positive charge?
Isotopes of an element have different numbers of protons.
False
What are the three main categories of elements in the periodic table?
Metals, Non-metals, Metalloids
Group 1 elements are known as ______ Metals.
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Which of the following elements is a halogen?
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How many valence electrons do alkaline earth metals have?
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Electrons are found in ______ around the nucleus of an atom.
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Match the group to its correct description:
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Study Notes
Atom Structure
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Protons, Neutrons, and Electrons
- Protons are positively charged particles located in the nucleus.
- Neutrons are neutral particles located in the nucleus.
- Electrons are negatively charged particles that orbit the nucleus.
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Atomic Mass Unit (amu)
- Protons and neutrons each have a mass of approximately 1 amu.
- Electrons have a very small mass, almost negligible.
Isotopes
- Definition: Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
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Properties:
- Isotopes of the same element share similar chemical properties but can have slightly different physical properties.
- This difference in physical properties can be attributed to the variation in mass caused by different numbers of neutrons.
Periodic Table Organization
- Invention: Dmitri Mendeleev invented the periodic table in the 1800s.
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Main Categories:
- Metals: Elements on the left side of the periodic table that are generally shiny, malleable, ductile, good conductors of heat and electricity.
- Non-metals: Elements on the right side of the periodic table that are generally not shiny, not malleable, not ductile, poor conductors of heat and electricity.
- Metalloids (semimetals): Elements found along the border between metals and non-metals, possessing properties of both.
Periodic Table Structure
- Periods (Horizontal Rows): Elements in the same period have the same number of electron shells or energy levels.
- Groups/Families (Vertical Columns): Elements in the same group have similar chemical properties due to sharing the same number of electrons in their outermost shell, also known as valence electrons.
Key Groups
Group 1: Alkali Metals
- Examples: Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), Francium (Fr)
- Valence Electrons: 1
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Physical Properties:
- Solid at room temperature
- Shiny, silvery color
- Soft metals
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Chemical Properties:
- Highly reactive
- React with water to produce hydrogen gas
- Exist in nature only as compounds
- Lose 1 electron to form +1 ions
Group 2: Alkaline Earth Metals
- Examples: Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), Radium (Ra)
- Valence Electrons: 2
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Physical Properties:
- Solid, denser than Group 1 metals
- Metallic
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Chemical Properties:
- Reactive, although less than Group 1 metals
- Exist in nature only as compounds
- Lose 2 electrons to form +2 ions
Group 17: Halogens
- Examples: Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At), Tennessine (Ts)
- Valence Electrons: 7
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Physical Properties:
- Non-metals
- Varied states:
- Fluorine (F) is a yellow gas
- Chlorine (Cl) is a yellow-green gas
- Bromine (Br) is a red-brown liquid
- Iodine (I) is a violet/black solid
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Chemical Properties:
- Highly reactive and corrosive
- Exist in nature only as compounds
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Description
Explore the fundamentals of atom structure, including protons, neutrons, electrons, and isotopes. This quiz examines atomic mass units and the organization of the periodic table. Understand how isotopes differ in physical properties while maintaining similar chemical characteristics.