Across
- 1. Bond: two pairs of electrons are shared
- 3. electrons: shield the valence electrons from the nucleus
- 5. negatively charged
- 7. Charge: determines how plausible a lewis structure is
- 8. length:smaller bonds have larger bond lengths
- 9. Electrons: electrons in the highest occupied energy level of an atom
- 11. Bonds: are less likely to undergo chemical change than a weaker bond
- 13. Series: a group of ions all containing the same amount of electrons
- 15. Bonds: unequal sharing of electrons
- 17. exception to octet rule as it only requires 4 electrons to be full
- 22. are shared in pairs
- 23. Polarity: nonpolar or polar bond
- 26. Energy: energy required to completely separate a mole of a solid ionic compound into its gaseous ions
- 27. Energy: amount of energy necessary to remove an electron from an isolated neutral atom in the gaseous state
- 29. effective nuclear charge taking into account attraction and repulsions
- 31. positively charged
Down
- 2. exception to octet rule as it only requires 6 electrons to be full
- 4. Bonds: usually occur in molecular compounds such as metals and non-metals
- 6. Bond: one pair of electrons are shared
- 10. Geometry: 3D geometry of a molecule
- 12. ionization energy: energy needed to remove the first electron
- 14. ability of a nucleus to attract an electron in a covalent bond to itself
- 16. Rule: nonmetals will share electrons to acquire 8 total valence rules
- 18. organic molecule present in aromatic compounds
- 19. Dot Structures: drawing to represent valence electrons
- 20. Radius: determined from distance between nuclei in ionic compounds
- 21. Bonds: electrons are shared equally between atoms
- 24. Structures: valid electrons structures to describe the bonding in a moleule
- 25. Radii: half the distance between the nuclei of two like atoms
- 28. Electrons: largely responsible for chemical properties of an element
- 30. Shells: only occur in period 3 and below