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Questions and Answers
What distinguishes isotopes of the same element from each other?
What distinguishes isotopes of the same element from each other?
Which particle in an atom carries a positive charge?
Which particle in an atom carries a positive charge?
How do metal atoms typically form ions?
How do metal atoms typically form ions?
What is the mass of an electron compared to protons and neutrons?
What is the mass of an electron compared to protons and neutrons?
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Which of the following formulas represents a compound ionic bond?
Which of the following formulas represents a compound ionic bond?
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Which ion is formed when a non-metal atom gains electrons?
Which ion is formed when a non-metal atom gains electrons?
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What is the typical electron arrangement for an atom with eight electrons in its outer shell?
What is the typical electron arrangement for an atom with eight electrons in its outer shell?
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Which of the following correctly represents the hydroxide ion?
Which of the following correctly represents the hydroxide ion?
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What determines the element of an atom?
What determines the element of an atom?
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Ions have the same number of protons and a different number of neutrons compared to their neutral atoms.
Ions have the same number of protons and a different number of neutrons compared to their neutral atoms.
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What is the charge of a neutron?
What is the charge of a neutron?
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Atoms in groups 1 and 2 typically _____ electrons to form ions.
Atoms in groups 1 and 2 typically _____ electrons to form ions.
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Match the following compound ions with their formulas:
Match the following compound ions with their formulas:
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Which ion is formed from an atom of ammonium?
Which ion is formed from an atom of ammonium?
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Electrons have a mass greater than neutrons.
Electrons have a mass greater than neutrons.
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What is the average mass of an element based on?
What is the average mass of an element based on?
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What is the relative atomic mass (RAM) of chlorine, given the isotopes 35Cl (75.77% abundance) and 37Cl (24.23% abundance)?
What is the relative atomic mass (RAM) of chlorine, given the isotopes 35Cl (75.77% abundance) and 37Cl (24.23% abundance)?
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Relative formula mass (RFM) and relative molecular mass (RMM) refer to the same concept.
Relative formula mass (RFM) and relative molecular mass (RMM) refer to the same concept.
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What is the formula used to calculate the relative formula mass (RFM) of a compound?
What is the formula used to calculate the relative formula mass (RFM) of a compound?
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The relative atomic mass reflects the abundance weighted average of __________.
The relative atomic mass reflects the abundance weighted average of __________.
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Match the following elements with their relative atomic masses:
Match the following elements with their relative atomic masses:
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What does a dot and cross diagram represent?
What does a dot and cross diagram represent?
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Hydrogen must have 8 electrons in its outer shell according to the octet rule.
Hydrogen must have 8 electrons in its outer shell according to the octet rule.
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What are the valence electron counts for carbon and hydrogen in methane (CH₄)?
What are the valence electron counts for carbon and hydrogen in methane (CH₄)?
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In magnesium oxide (MgO), magnesium loses _____ electrons to form Mg²⁺.
In magnesium oxide (MgO), magnesium loses _____ electrons to form Mg²⁺.
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Match what these atoms gain or lose electrons to become
Match what these atoms gain or lose electrons to become
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Study Notes
Atomic Structure
- Atoms are mostly empty space
- The number of protons determines the element
- Ions are charged atoms; same number of protons but different number of electrons
- Isotopes are atoms with the same number of protons but different numbers of neutrons
Subatomic Particles
- Protons: positive charge, mass 1
- Neutrons: no charge, mass 1
- Electrons: negative charge, negligible mass
Atomic Mass
- Average atomic mass includes all isotopes
- Relative atomic mass is the weighted average mass of all isotopes
Ions
- Metal atoms lose electrons and form positive ions (cations)
- Non-metal atoms gain electrons and form negative ions (anions)
- Atoms in groups 1 and 2 lose electrons to form +1 and +2 ions respectively
- Atoms in groups 6 and 7 gain electrons to form -2 and -1 ions respectively
Compound Ions
- Groups of atoms with an overall charge
- Examples: hydroxide (OH⁻), nitrate (NO₃⁻), sulfate (SO₄²⁻), phosphate (PO₄³⁻), ammonium (NH₄⁺)
Chemical Formulas
- Represents the composition of compounds
- Shows the number and type of atoms in a compound
- Examples of writing chemical formulas:
- Sodium hydroxide: NaOH
- Ammonium nitrate: NH₄NO₃
- Potassium sulfate: K₂SO₄
- Calcium phosphate: Ca₃(PO₄)₂
- Aluminum Oxide: Al₂O₃
- Lithium Bromide: LiBr
Electron Arrangement
- Electrons orbit the nucleus in shells or energy levels
- The arrangement of electrons determines an element's chemical properties
- The first shell holds a maximum of two electrons, the second holds a maximum of eight and so on.
- Example: Magnesium (Mg) electron configuration: 2,8,2
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Description
This quiz explores the fundamental concepts of atomic structure, including protons, neutrons, electrons, ions, and isotopes. Test your knowledge on how these particles contribute to the properties of elements and compounds. Ideal for high school chemistry students.
