1. Arrange students into groups. Each group needs at least ONE person who has a mobile device.
2. If their phone camera doesn't automatically detect and decode QR codes, ask students to
4. Cut them out and place them around your class / school.
1. Give each group a clipboard and a piece of paper so they can write down the decoded questions and their answers to them.
2. Explain to the students that the codes are hidden around the school. Each team will get ONE point for each question they correctly decode and copy down onto their sheet, and a further TWO points if they can then provide the correct answer and write this down underneath the question.
3. Away they go! The winner is the first team to return with the most correct answers in the time available. This could be within a lesson, or during a lunchbreak, or even over several days!
4. A detailed case study in how to set up a successful QR Scavenger Hunt using this tool can be found here.
Question | Answer |
| 1. Are there few or many electrons in the outermost energy level of metals? | few | 2. What is the difference between malleability and ductility? | bend vs. stretch | 3. What are the two types of covalent bonds? | pure covalent and polar covalent | 4. How does electronegativity change as you move from left to right across the periodic table? | increase | 5. What type of elements form ionic bonds? | metals and nonmetals | 6. Give an example of a polar covalent bond? | answers may vary | 7. How can we use the periodic table to help us determine the type of bonding between atoms? | Trends in electronegativity and metals vs non metals | 8. Why do we only consider Valence electrons in drawing Lewis structures? | they are the ones that react | 9. The relative ability of an atom in a molecule to attract electrons to itself is called the atoms ___________. | electronegativity | 10. What is a dipole moment?; draw an example. | electrical effect that occurs in molecules with separate centers of positive and negative charge. | 11. What does it mean when we say that in forming bonds, atoms try to achieve an electron configuration of a noble gas? | most stable configuration. | 12. Double point questions! Why are cations always smaller than the atoms from which they were formed? | loss of e so one valence shell is lost | 13. Explain the difference between the duet and the octet rule. Give an example of an atom that follows each. | H and O | 14. Write the Lewis structure for Sr. | see notes | 15. Write the Lewis structure for C2F6. | see notes | 16. Write the Lewis structure for N2H4. | see notes | 17. Write the Lewis structure for the sulfate ion. | SO4 2- | 18. What does it mean for a molecule to exhibit resonance? | more than one lewis structure | 19. Write the Lewis structure for the barium ion. | Ba2+ | 20. What general principles determine the molecular structure (shape) of a molecule? | how many e pairs surround, which pairs used for bonding | 21. Come to the classroom and build a model of one of the molecules listed by the parts kit. | see models |
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