Across
- 4. Located in the nucleus of the atom and bear a neutral charge. Page 25
- 6. To change reversibly from a fluid (sol) state to a more solid (gel)state. Page 30
- 7. Energy that is directly involved in moving matter. Page 24
- 14. When atoms with 6 or 7 valence electrons attracts electrons strongly. Page 34
- 15. Unequal electron pair sharing. Page 34
- 17. To express the concentration of a solution. Page 29
- 18. A listing of the known elements and helps to explain their properties. Page 25
- 19. The atom that gains one or more electrons is the electron acceptor. Page 32
- 20. Energy in action. Page 24
- 22. Located in the nucleus of the atom and bear a positive charge. Page 25
- 26. The atom that loses electrons is the electron donor. Page 32
- 27. A sentence describing what happens in a reaction. Page 35
- 30. Substances present in smaller amounts. Page 29
- 32. They are the basis of all reactions in which food fuels are broken down for energy. Page 36
- 33. Atom that has the same number of protons but different numbers of neutrons. Page 27
- 38. Electrons forming the electron cloud around the nucleus of an atom that occupy regions. Page 31
- 39. A chemical bond between atoms formed by the transfer of one or more electrons from one atom to the other. Page 32
- 41. Homogeneous mixtures of components that may be gases, liquid or solids. Page 29
- 42. Substances present in the greatest amount. Page 29
- 43. Stored in the bonds of chemical substances. Page 24
- 46. Formed when a hydrogen atom, is linked to an electronegative atom. Page 34
- 47. The sum of masses of its protons and neutrons. Page 27
- 49. Each element designates by one or two letter. Page 25
- 50. Substances compound of two or more compounds. Page 29
- 51. Anything that occupies space and has mass. Page 24
Down
- 1. results from the movement of charged particles. Page 24
- 2. Energy that travels in waves. Page 24
- 3. When smaller particles are bonded to form complex molecules. Page 36
- 5. Energy is stored and inactive. Page 24
- 8. To convert energy from one form to another. Page 24
- 9. Reacting substances in a chemical reaction. Page 35
- 10. Substances that increases the rate of chemical reactions without becoming chemically charged. Page 38
- 11. When bonds are broken in larger molecules, resulting in smaller, less complex molecules. Page 36
- 12. Located in the centre of the atoms and consist of protons and neutrons. Page 25
- 13. bonds - An energy relationship between the electrons of the reacting atoms, and it is made or brake in trillionth of a second. Page 31
- 16. Atoms with one or two valence shell electrons. Page 34
- 21. Isotopes that exhibit reactivity behavior. Page 28
- 23. Regions around the nucleus in which a given electron or electron pair is likely to be found. Page 26
- 24. An average of the relative weights (mass numbers) of all the isotopes of an element. Page 28
- 25. Molecules that are formed from covalent bonds and are electronically balanced. Page 33-34
- 28. Clusters of even smaller particles called protons, neutrons and electrons. Page 24
- 29. A combination of two or more atoms held together by chemical bond. Page 28
- 31. Located on the shell of the atom and has a negative charge. Page 25
- 34. Heterogeneous mixtures, which means that the composition is dissimilar in different arears of the mixture. Page 30
- 35. Heterogenous mixtures with large, often visible solutes that tend to settle out. Page 30
- 36. Equal to the number of protons in its nucleus. Page 27
- 37. When two or more different kinds of atoms bond. Page 28
- 40. Electron sharing produces molecules. Page 32
- 44. The process of the atomic decay. Page 28
- 45. Equal to its atomic weight or molecular weight. Page 29
- 48. Predicting the chemical behavior of atoms. Page 26