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- 1. Multiple ChoiceElements such as Silicon, diamond and graphite. Compounds include SiO2simple covalent moleculesmetallicionicgiant covalent
- 2. Multiple ChoiceMelting points are very high – a large amount of energy is needed to break all the covalent bondssimple covalent moleculesmetallicionicgiant covalent
- 3. Multiple ChoiceLattice structure in which all atoms are joined to others by covalent bondssimple covalent moleculesmetallicionicgiant covalent
- 4. Multiple Choice
A fixed number of atoms bonded together, if bonds are broken they would have different properties.
Examples include H2O , NH3 , PCl5
simple covalent molecules
metallic
ionic
giant covalent
- 5. Multiple ChoiceFormulae of these might include H2O
each molecule contains 1 O and 2H atomssimple covalent moleculesmetallicionicgiant covalent - 6. Multiple Choice
What structure is shown in the diagram?DiamondGraphiteCarbon fiberCarbon nanotubes - 7. Multiple ChoiceCovalent compoundsShare electronstransfer electronscontain a sea of electronsconduct electricity
- 8. Multiple ChoiceWhy is diamond strong?It's made of carbonIt doesn't conduct electricityIt forms 4 strong covalent bondsSo it can cut glass
- 9. Multiple ChoiceWhy is graphite so soft?A. The atoms are arranged in hexagons in layers that are held together stronglyB. The atoms are arranged in hexagons in layers that are held together weaklyC. Carbon is strongly bonded to 3 other carbon atoms.D. Carbon is weakly bonded to 3 other carbon atoms.
- 10. Multiple ChoiceWhat element are diamond and graphite made up of?A. SodiumB. CarbonC. Carbon dioxideD. Silicon
- 11. Multiple ChoiceWhy does graphite conduct electricity?Ions are free to move to carry the chargeAoms can moveFree electrons that can carry the charge
- 12. Multiple Choice8. What type of Chemical Bonding is best defined as 'SHARING OF ELECTRONS '?a) Intermolecular Bondingb) Metallic Bondingc) Ionic Bondingd) Covalent Bonding
- 13. Multiple ChoiceGraphite is a good conductor becauseall electrons are free moving electronsfree delocalization of electrons in its 3D lattice structurefree delocalized electrons in a 2D layered structurecovalently bonded layers allow electricity to flow
- 14. Multiple ChoiceDiamond has a very high melting point due toStrong covalent bonds between carbon atoms in a layered structureAll carbon atoms are covalently bonded to 3 other carbonsStrong ionic bonds in a lattice structureCarbon atom covalently bonded to 4 other Carbons in a giant structure
- 15. Multiple ChoiceWhat structure is shown in the diagram?DiamondGraphitefullerene
- 16. Multiple ChoiceWhat structure is shown in the diagram?DiamondGraphitefullerene
- 17. Multiple ChoiceConduct electricitydiamondgraphiteboth
- 18. Multiple Choiceused in cutting tools like drill bitsdiamondgraphitefullerene
- 19. Multiple Choice
Each carbon in diamond forms ______ bonds
1
2
3
4
- 20. Multiple Choice
Each carbon is graphite forms _____ bonds
1
2
3
4
- 21. Multiple ChoiceWhat two types of atoms make a covalent bond?2 Nonmetals1 Nonmetal and 1 Metal2 Metals2 Noble Gases
- 22. Multiple Choice
How are covalent bonds explained?
When one atom takes the other atom's electron
A shared pair of electrons between bonding atoms
When the two nucleus merge
When the neutrons leave the nucleus
- 23. Multiple ChoiceWhat region of the periodic table contains atoms that form covalent bonds?the left sidethe middlethe right sidetop left
- 24. Multiple ChoiceIs carbon considered a metal or a non-metal?metalnonmetalother
- 25. Multiple Choice
What type of bonding holds together the atoms in graphite?
ionic
covalent
metallic
- 26. Multiple Choice
Why is graphite so soft and slippery?
It is made of layers of atoms
It is made of small molecules
It is an ionic compound
- 27. Multiple Choice
The atoms in diamond are joined together by which type of bonds?
Ionic
Covalent
Metallic
- 28. Multiple Choice
Diamond is suitable for the cutting end of a drill bit because it is
hard
shiny
soft
- Answer choicesTagsAnswer choicesTags