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Chemistry-Chapter 12-Chemical Bonding
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Bond: Also known as a chemical bond. The force that holds two or more atoms together and makes them function as a unit.
Bond Energy: The energy required to break a given chemical bond.
Ionic Bonding: The attraction between oppositely charged ions.
Ionic Compound: A compound that results when a metal reacts with a nonmetal to form cations and anions.
Covalent Bonding: A type of bonding in which atoms share electrons.
Polar Covalent Bond: A covalent bond in which the electrons are not shared equally because one atom attracts the shared electrons more than the other atom.
Electronegativity: The tendency of an atom in a molecule to attract shared electrons to itself.
Dipole Moment: A property of a molecule in which the charge distribution can be represented by a center of positive charge and a center of negative charge.
Lewis Structure: A representation of a molecule or polyatomic ion showing how valence electrons are arranged among the atoms in the molecule or ion.
Duet Rule:Rule that Hydrogen follows that it needs two electrons to be stable.
Octet Rule:Rule that elements follow that they need eight electrons to fill their orbitals to become stable.
Bonding Pair: A pair of electrons that are shared between two atoms forming a covalent or polar-covalent bond.
Lone pair: Also known as unshaired pairs. Electron pairs in a Lewis structure that are not involved in bonding.
Single Bond: A covalent or polar covalent bond in which one pair of electrons is shared by two atoms.
Double Bond: A covalent or polar covalent bond in which two pairs of electrons are shared by two atoms.
Triple Bond: A covalent or polar covalent bond in which three pairs of electrons are shared by two atoms.
Resonance: A condition occurring when more than one valid Lewis Structure can be written for a particular molecule.
Molecular Structure: The three-dimensional arrangement of atoms in a structure.
Linear Structure: All atoms in a line.
Trigonal Planar Structure: All four atoms in the same plane with 120 degree bond angles.
Tetrahedral Structure: A tetrahedron
Valence Shell Electron Pair Repulsion Model: A model used to predict molecular geometry. Based on the idea that pairs of electrons surrounding an atom repel each other and that the atoms in a molecule are positioned to minimize this repulsion.
Trigonal Pyramid: Has a tetrahedral arrangement of electron pairs but not a tetrahedral arrangement of atoms. One side is different from the other three
Chemistry-Chapter 12-Chemical Bonding
Across:4. | Has a tetrahedral arrangement of electron pairs but not a tetrahedral arrangement of atoms. One side is different from the other three | 10. | A property of a molecule in which the charge distribution can be represented by a center of positive charge and a center of negative charge. | 12. | The three-dimensional arrangement of atoms in a structure. | 16. | The attraction between oppositely charged ions. | 17. | Rule that Hydrogen follows that it needs two electrons to be stable. |
| 19. | A compound that results when a metal reacts with a nonmetal to form cations and anions. | 21. | A covalent or polar covalent bond in which three pairs of electrons are shared by two atoms. | 22. | Also known as unshaired pairs. Electron pairs in a Lewis structure that are not involved in bonding. | 23. | A type of bonding in which atoms share electrons. |
| | Down:1. | A pair of electrons that are shared between two atoms forming a covalent or polar-covalent bond. | 2. | A model used to predict molecular geometry. Based on the idea that pairs of electrons surrounding an atom repel each other and that the atoms in a molecule are positioned to minimize this repulsion. | 3. | A covalent or polar covalent bond in which one pair of electrons is shared by two atoms. | 5. | A condition occurring when more than one valid Lewis Structure can be written for a particular molecule. | 6. | A representation of a molecule or polyatomic ion showing how valence electrons are arranged among the atoms in the molecule or ion. | 7. | The energy required to break a given chemical bond. | 8. | The tendency of an atom in a molecule to attract shared electrons to itself. |
| 9. | A tetrahedron | 11. | All atoms in a line. | 13. | All four atoms in the same plane with 120 degree bond angles. | 14. | A covalent or polar covalent bond in which two pairs of electrons are shared by two atoms. | 15. | Also known as a chemical bond. The force that holds two or more atoms together and makes them function as a unit. | 18. | Rule that elements follow that they need eight electrons to fill their orbitals to become stable. | 20. | A covalent bond in which the electrons are not shared equally because one atom attracts the shared electrons more than the other atom. |
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© 2014
PuzzleFast.com, Noncommercial Use Only
Chemistry-Chapter 12-Chemical Bonding
Across:4. | Has a tetrahedral arrangement of electron pairs but not a tetrahedral arrangement of atoms. One side is different from the other three | 10. | A property of a molecule in which the charge distribution can be represented by a center of positive charge and a center of negative charge. | 12. | The three-dimensional arrangement of atoms in a structure. | 16. | The attraction between oppositely charged ions. | 17. | Rule that Hydrogen follows that it needs two electrons to be stable. |
| 19. | A compound that results when a metal reacts with a nonmetal to form cations and anions. | 21. | A covalent or polar covalent bond in which three pairs of electrons are shared by two atoms. | 22. | Also known as unshaired pairs. Electron pairs in a Lewis structure that are not involved in bonding. | 23. | A type of bonding in which atoms share electrons. |
| | Down:1. | A pair of electrons that are shared between two atoms forming a covalent or polar-covalent bond. | 2. | A model used to predict molecular geometry. Based on the idea that pairs of electrons surrounding an atom repel each other and that the atoms in a molecule are positioned to minimize this repulsion. | 3. | A covalent or polar covalent bond in which one pair of electrons is shared by two atoms. | 5. | A condition occurring when more than one valid Lewis Structure can be written for a particular molecule. | 6. | A representation of a molecule or polyatomic ion showing how valence electrons are arranged among the atoms in the molecule or ion. | 7. | The energy required to break a given chemical bond. | 8. | The tendency of an atom in a molecule to attract shared electrons to itself. |
| 9. | A tetrahedron | 11. | All atoms in a line. | 13. | All four atoms in the same plane with 120 degree bond angles. | 14. | A covalent or polar covalent bond in which two pairs of electrons are shared by two atoms. | 15. | Also known as a chemical bond. The force that holds two or more atoms together and makes them function as a unit. | 18. | Rule that elements follow that they need eight electrons to fill their orbitals to become stable. | 20. | A covalent bond in which the electrons are not shared equally because one atom attracts the shared electrons more than the other atom. |
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© 2014
PuzzleFast.com, Noncommercial Use Only