Questions and Answers
The number of valence electrons found in an atom of a Group A element is equal to:
How many valence electrons are in the electron-dot structures for the elements in group 3A(13)?
How many valence electrons does nitrogen have?
How many electrons will aluminum gain or lose when it forms an ion?
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What is the symbol for the ion with 19 protons and 18 electrons?
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The number of electrons in an ion with 20 protons and an ionic charge of 2+ is:
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Elements in group 2A(2) of the periodic table form ions with a charge of:
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What is the correct formula for the oxide ion?
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An ionic compound:
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The correct formula for the compound formed from Mg and S is:
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Which one of the following compounds contains an ion with a 3+ charge?
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Which one of the following elements forms two or more ions with different ionic charges?
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What is the correct formula for lead (IV) oxide?
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The name of Al2(SO4)3 is:
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The formula for copper (II) sulfate is:
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What are the ions present in Al2(SO4)3?
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What is the charge on the Fe ion in the molecule Fe2(CO3)3?
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The formula for a compound containing ammonium ion and phosphate ion is:
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In a molecule with covalent bonding:
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The name of the compound SO3 is:
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The formula for a molecule formed from N and Cl would be:
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What is the formula of carbon tetraiodide?
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Which of the following elements does NOT exist as a diatomic molecule?
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How many valence electrons are in the electron-dot structure of H2O?
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How many lone pairs of electrons are in the electron-dot structure of H2O?
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The ability of an atom to attract the shared electrons in a covalent bond is:
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Which of the following substances contains a polar covalent bond?
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Ionic bonding is expected in which of these compounds?
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The shape of the carbon tetrachloride molecule is:
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The electron group geometry of NH3 molecule is:
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The carbon tetrachloride molecule, CCl4, is:
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The strongest interactions between molecules of ammonia (NH3) are:
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The strongest interactions in the compound sodium fluoride, NaF, are examples of:
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Study Notes
Valence Electrons and Ion Charges
- The number of valence electrons in a Group A element equals its group number.
- Group 3A(13) elements have three valence electrons.
- Nitrogen has five valence electrons.
- Aluminum loses three electrons to form a +3 ion.
Ionic Charges and Compounds
- The ion with 19 protons and 18 electrons is K+.
- An ion with 20 protons and a 2+ charge has 18 electrons.
- Group 2A(2) elements form ions with a 2+ charge.
- The formula for the oxide ion is O2-.
- Ionic compounds have a net charge of zero.
- The formula for magnesium and sulfur compound is MgS.
- FeCl3 contains an ion with a 3+ charge.
- Iron (Fe) can form multiple ions with different charges.
- Lead (IV) oxide's correct formula is PbO2.
Chemical Formulas and Naming
- Al2(SO4)3 is named aluminum sulfate.
- The formula for copper (II) sulfate is CuSO4.
- The ions present in Al2(SO4)3 are Al3+ and SO4 2-.
- The charge on the Fe ion in Fe2(CO3)3 is 3+.
- The compound containing ammonium ion and phosphate ion is (NH4)3PO4.
Covalent Bonds
- In covalent bonding, atoms are held together by shared electrons.
- The compound SO3 is named sulfur trioxide.
- The formula for a compound of nitrogen and chlorine is NCl3.
- The formula for carbon tetraiodide is CI4.
Molecular Structure
- Carbon does not exist as a diatomic molecule while H2, N2, Cl2, and O2 do.
- H2O has eight valence electrons in its electron-dot structure.
- H2O has two lone pairs of electrons shown in its structure.
- Electronegativity indicates an atom's ability to attract shared electrons in a bond.
- NH3 contains a polar covalent bond.
- Ionic bonding predominantly occurs in KF.
Molecular Geometry
- The shape of carbon tetrachloride (CCl4) is tetrahedral.
- NH3 also has a tetrahedral electron group geometry.
- CCl4 is a nonpolar molecule with polar bonds.
Intermolecular Forces
- The strongest interactions in ammonia (NH3) are hydrogen bonds.
- Sodium fluoride (NaF) has the strongest interactions due to ionic bonds.
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Description
Test your knowledge of valence electrons and electron-dot structures with these flashcards from CHEM 101 Chapter 6. Each question challenges you to recall essential concepts related to group A elements and their properties. Perfect for final exam preparation!