Chemical Bonding

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Across
  1. 5. The hypothetical charge on an atom in a molecule, assuming equal sharing of electrons in bonds.
  2. 7. A molecular orbital that weakens the bond between two atoms and has higher energy than the atomic orbitals from which it was formed.
  3. 9. A measure of the separation of positive and negative charges in a molecule.
  4. 12. A diagram showing the bonding between atoms and the lone pairs of electrons in a molecule using dots to represent electrons.
  5. 14. A bond formed by the direct overlap of atomic orbitals along the internuclear axis.
  6. 20. Orbitals that belong to the entire molecule rather than to a single atom, formed by the combination of atomic orbitals.
  7. 23. The concept that electron pairs around a central atom will arrange themselves to be as far apart as possible, minimizing repulsive forces.
  8. 25. A bond formed by the side-by-side overlap of atomic orbitals, with electron density above and below the plane of the nuclei.
  9. 26. Orbitals that are formed by the mixing of atomic orbitals on the same atom to form equivalent orbitals for bonding.
  10. 27. The concept where a molecule is represented by two or more structures (resonance structures) that together depict the bonding in the molecule.
  11. 28. The ability of an atom to attract electrons in a chemical bond.
  12. 29. A bond formed by the transfer of electrons from one atom to another, leading to the formation of positively and negatively charged ions.
  13. 30. Valence Shell Electron Pair Repulsion theory, used to predict the geometry of molecules based on the repulsion between electron pairs.
Down
  1. 1. A chemical bond formed by the sharing of electron pairs between atoms.
  2. 2. The radius of an atom's ion in a crystal lattice, differing for cations and anions.
  3. 3. The energy change that occurs when an electron is added to a neutral atom to form a negative ion.
  4. 4. A three-dimensional arrangement of atoms or ions in a crystalline solid.
  5. 6. The outermost electrons of an atom, which are involved in forming chemical bonds.
  6. 8. The number of chemical bonds between a pair of atoms.
  7. 10. The three-dimensional arrangement of atoms in a molecule.
  8. 11. A covalent bond where the electrons are not shared equally, leading to partial charges.
  9. 13. The process by which atomic orbitals mix to form new hybrid orbitals with equivalent energy and shape.
  10. 15. The distribution of electrical charge over the atoms joined by the bond, which results in partial positive and negative charges.
  11. 16. The average distance between the nuclei of two bonded atoms.
  12. 17. The attractive force that holds atoms together in a molecule or compound.
  13. 18. A pair of valence electrons that are not shared with another atom and are found in the outermost electron shell.
  14. 19. Atoms combine by gaining, losing, or sharing electrons to achieve a stable octet in their valence shells.
  15. 21. The energy required to break one mole of bonds in a gaseous substance.
  16. 22. The energy required to break the bond between two covalently bonded atoms.
  17. 24. A weak bond between a hydrogen atom, which is covalently bonded to a more electronegative atom, and another electronegative atom.