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Questions and Answers
Which of the following describes the typical behavior of metal atoms when forming ions?
Which of the following describes the typical behavior of metal atoms when forming ions?
- Gain electrons to become negatively charged anions.
- Neither gain nor lose electrons, remaining neutral.
- Share electrons to form covalent compounds.
- Lose electrons to achieve a stable outer electron shell, forming positive cations. (correct)
Why do non-metal atoms typically gain electrons when forming ions?
Why do non-metal atoms typically gain electrons when forming ions?
- To lose energy and become less reactive.
- To decrease the number of protons in their nucleus.
- To achieve a full outer electron shell and become more stable. (correct)
- To balance the positive charge of the nucleus.
How does the number of valence electrons relate to an element's position on the periodic table and its tendency to form ions?
How does the number of valence electrons relate to an element's position on the periodic table and its tendency to form ions?
- The group number indicates the number of protons, predicting whether it will lose or gain electrons.
- The group number indicates the number of valence electrons, predicting whether it will lose or gain electrons. (correct)
- The period number indicates the number of electron shells, predicting the stability of the ion formed.
- The period number indicates the number of valence electrons, predicting the charge of the ion formed.
What characteristic defines an ionic bond?
What characteristic defines an ionic bond?
Which of the following best describes the arrangement of ions in an ionic lattice?
Which of the following best describes the arrangement of ions in an ionic lattice?
Magnesium (Mg) is in group 2 of the periodic table. What charge would you expect a magnesium ion to have?
Magnesium (Mg) is in group 2 of the periodic table. What charge would you expect a magnesium ion to have?
Oxygen (O) is in group 6 of the periodic table. What charge would you expect an oxygen ion to have?
Oxygen (O) is in group 6 of the periodic table. What charge would you expect an oxygen ion to have?
Consider a neutral atom with an electronic configuration of 2, 8, 7. What type of ion will it form, and what will be its charge?
Consider a neutral atom with an electronic configuration of 2, 8, 7. What type of ion will it form, and what will be its charge?
Sodium (Na) forms an ion with a +1 charge. Which of the following statements accurately describes what happens when sodium forms this ion?
Sodium (Na) forms an ion with a +1 charge. Which of the following statements accurately describes what happens when sodium forms this ion?
Which of the following elements is most likely to form an ionic bond with chlorine (Cl)?
Which of the following elements is most likely to form an ionic bond with chlorine (Cl)?
Why are noble gases generally unreactive?
Why are noble gases generally unreactive?
How does the electron configuration 2, 8, 6 influence the ionic behavior of an atom?
How does the electron configuration 2, 8, 6 influence the ionic behavior of an atom?
What happens to the number of protons, neutrons, and electrons when an atom of chlorine (Cl) becomes a chloride ion (Cl-)?
What happens to the number of protons, neutrons, and electrons when an atom of chlorine (Cl) becomes a chloride ion (Cl-)?
If element X is in Group 15 (also known as Group 5A) of the periodic table, what is the most likely charge of the ion it will form?
If element X is in Group 15 (also known as Group 5A) of the periodic table, what is the most likely charge of the ion it will form?
Consider the formation of potassium iodide (KI). Potassium (K) loses one electron, and iodine (I) gains one electron. Which statement accurately describes the resulting compound?
Consider the formation of potassium iodide (KI). Potassium (K) loses one electron, and iodine (I) gains one electron. Which statement accurately describes the resulting compound?
Flashcards
What is an ion?
What is an ion?
A charged atom or molecule due to the loss or gain of electrons.
What are metal cations?
What are metal cations?
Positively charged ions formed when metal atoms lose electrons.
Why do metals lose electrons?
Why do metals lose electrons?
They lose electrons to achieve a stable outer shell.
How to find valence electrons in a metal?
How to find valence electrons in a metal?
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What are non-metal anions?
What are non-metal anions?
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Why do non-metals gain electrons?
Why do non-metals gain electrons?
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How to find valence electrons in non-metals?
How to find valence electrons in non-metals?
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How are ions formed?
How are ions formed?
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What is an ionic bond?
What is an ionic bond?
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What is an ionic lattice?
What is an ionic lattice?
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The Octet Rule
The Octet Rule
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What are valence electrons?
What are valence electrons?
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Study Notes
- Atoms form ions by losing and gaining electrons
- An atom can be represented like a ball
Atomic Structure
- An atom contains a nucleus, neutrons, protons, and electrons
- Electrons are located in orbits
- The electronic configuration of an atom 2, 8, 1
- Valence electrons are the outer shell electrons
- Atoms are more stable with 8 valence electrons
Metal Atoms
- Metal atoms become ions by losing electrons
- Metals have 1, 2, or 3 valence electrons.
- Metals lose valence electrons to gain a stable outer shell
- Metal atoms are able to find out about the number of a metal atoms valence electrons via the periodic table
- Sodium is in group 1, it is a metal atom with 1 valence electron; therefore, it loses 1 electron to form a singly charged ion Na+
Non-Metal Atoms
- Non-metal atoms gain electrons to form ions
- Non-metals have 4, 6, or 7 valence electrons
- Non-metals gain valence electrons needed to gain a stable outer shell
- To determine the number of valence electrons in a non-metal atom, check the periodic table
- Oxygen is in group 8; it is a non-metal atom with 6 valence electrons, because it gains 2 electrons it forms the ion 02-
Formation of Ions via Elements on the Periodic Table
- Group 1 loses 1, Group 2 loses 2, transition metals usually lose 2
- Group 3 loses 3, Groups 4 and 5 do not form ions, Group 6 gains 2, and Group 7 gains 1
- Noble gases can't lose or gain ions
- Na+ and K+ are in Group 1
- Mg2+ and Ca2+ are in Group 2
- Cu2+ and Zn2+ are transition metals
- Al3+ is in Group 3
- The ions 02- and S2- are in Group 6
- F- and Cl- are in Group 7
Ionic Bonds and Lattices
- Ions have a charge, resulting in electrostatic attraction
- This is because opposite charges attract
- The two balls stick to each other...This phenomenon is the ionic bond
- Electrons move from Na atoms to Cl atoms
- Lots of ions are formed, those with opposite charge are attracted
- Ions form up into a regular arrangement or ionic lattice
- Nearest neighbors in an ionic lattice all have the opposite charge
- Each positive ion is surrounded by negative ions and vice versa
- Ionic lattices contain lots of ionic bonds
- The whole structure, ionic lattice, is tightly held together
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Description
Atoms form ions by gaining or losing electrons, and can be represented like a ball. Metal atoms lose electrons to form ions, while non-metal atoms gain electrons. The number of valence electrons can be determined via the periodic table.
