Across
- 6. is usually the compound’s empirical formula for ionic compounds.
- 8. is often useful to know the percentage by mass of a particular element in a chemical compound.
- 14. polyatomic ions that contain oxygen.
- 15. is numerically equal to its molar mass, so a compound’s molecular formula can also be found given the compound’s empirical formula and its molar mass.
- 17. is a certain type of molecular compound.
- 18. involves combining the names of the compound’s positive and negative ions.
- 19. consists of the symbols for the elements combined in a compound, with
- 21. indicates the relative number of atoms of each kind in a chemical compound.
- 22. An ionic compound composed of a cation and the anion from an acid
- 23. can be assigned to atoms in order to keep track of electron distributions in molecular as well as ionic compounds.
- 24. To distinguish the ions formed by such elements.
Down
- 1. is the actual formula of a molecular compound.
- 2. showing the smallest whole-number mole ratio of the different atoms in the compound.
- 3. Shows how the atoms in each ion are bonded together.
- 4. has an oxidation number of +1 in all compounds containing elements that are more electronegative than it but has an oxidation number of –1 with metals.
- 5. are acids that consist of two elements,usually hydrogen and a halogen.
- 7. numerically equal to its formula mass.
- 9. compounds composed of two elements
- 10. The mass of a water molecule
- 11. are acids that contain hydrogen, oxygen,and a third element (usually a nonmetal).
- 12. is the sum of the average atomic masses of all atoms represented in its formula.
- 13. are bound together in a group and carry a characteristic charge.
- 16. usually has an oxidation number of –2.
- 20. has an oxidation number of –1 in all its compounds because it is the most electronegative element.