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Questions and Answers
What is the relative mass of an electron compared to protons and neutrons?
What is the relative mass of an electron compared to protons and neutrons?
Isotopes have different atomic numbers but the same mass number.
Isotopes have different atomic numbers but the same mass number.
False
What is the role of Mendeleev in the development of the Periodic Table?
What is the role of Mendeleev in the development of the Periodic Table?
He arranged elements by properties and atomic mass, and left gaps predicting undiscovered elements.
Group 1 elements are known as _______ metals.
Group 1 elements are known as _______ metals.
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Match the following groups with their characteristics:
Match the following groups with their characteristics:
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Study Notes
Atomic Structure
- Atoms are the smallest unit of matter
- Molecules are a group of atoms bonded together
- Atoms consist of:
- Protons: Positive charge, located in the nucleus, relative mass 1
- Neutrons: No charge, located in the nucleus, relative mass 1
- Electrons: Negative charge, located in shells, relative mass ~0
- Atomic number: Number of protons in an atom
- Mass number: Sum of protons and neutrons
- Isotopes: Atoms of the same element with the same number of protons but different number of neutrons
- Relative atomic mass (Ar): Average mass of isotopes, weighted by their abundance
- Calculate Ar using isotope abundances
The Periodic Table
- Mendeleev arranged elements by properties and atomic mass
- He left gaps predicting undiscovered elements
- Modern periodic table is arranged in order of increasing atomic number
- Groups: Vertical columns; Periods: Horizontal rows
- Metals are on the left-hand side; non-metals are on the right-hand side
- Group number indicates the number of electrons in the outer shell
- Period number indicates the number of electron shells
- Elements in the same group have similar chemical properties
Ionic and Covalent Bonding
- Ionic bonding: Transfer of electrons between metals and nonmetals, forming positive (metal) and negative (non-metal) ions.
- Draw dot-cross diagrams for ionic compounds
- Covalent bonding: Sharing of electrons between nonmetals
- Draw dot-cross diagrams for covalent compounds
- Common ion charges are important to memorize:
- Group 1, 2, and 3 metals form positive ions
- Group 5, 6, and 7 non-metals form negative ions
- Specific ions should be known (e.g., charges for given ions)
Group 1 (Alkali Metals)
- React with water to produce hydrogen gas and an alkali
- Reactivity increases down the group
- Use reactivity trends to predict properties of other alkali metals
Group 7 (Halogens)
- Colors, physical states, and reactivity trends (decrease down the group) should be known
- Displacement reactions demonstrate reactivity trends
- Use reactivity trends to predict halogen properties
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Description
Test your knowledge on atomic structure and the periodic table with this quiz. Covering topics such as protons, neutrons, isotopes, and the arrangement of elements, this quiz is essential for understanding these fundamental concepts in chemistry.
