What is the type of bond that is related to group 14 elements’ melting points?
Carbon is a non-metal
Silicon and germanium are metals
Tin and Lead are metalloids
7. Multiple Choice
1 minute
1 pt
What is the type of bond that is related to group 14 elements’ melting points?
Silicon and germanium are metalloids
Carbon is a metal
Tin and Lead are metalloids
8. Multiple Choice
1 minute
1 pt
What is the type of bond that is related to group 14 elements’ melting points?
Tin and Lead are metals
Silicon and germanium are non-metals
Carbon is a metalloids
9. Multiple Choice
1 minute
1 pt
Change in electrical conductivity when going down group 14 is _________.
Increases, because the atomic radius causes the valence electrons to become more delocalised.
Increases, the size of atom is increasing, the attractive force between the atom will decrease.
Increases, the atomic radius causes the valence electrons to become more delocalised.
Increases, the atomic forces within the larger molecules are strong.
10. Multiple Choice
1 minute
1 pt
Change in electrical conductivity when going down group 14 is _________.
Increases, because the properties of the elements change from non-metallic to metallic.
Increases, the size of atom is increasing, the attractive force between the atom will decrease.
Increases, the atomic radius causes the valence electrons to become more delocalised.
Increases, the atomic forces within the larger molecules are strong.
11. Multiple Choice
1 minute
1 pt
Change in electrical conductivity when going down group 14 is _________.
Increases, because the metallic character increases.
Increases, the size of atom is increasing, the attractive force between the atom will decrease.
Increases, the atomic radius causes the valence electrons to become more delocalised.
Increases, the atomic forces within the larger molecules are strong.
12. Multiple Choice
1 minute
1 pt
C, (graphite) is a good conductor because __________
due to the mobility of the electrons in its outer valence shells.
each carbon atom forms four covalent bonds with other carbon atoms.
there are covalent bonds between the layers.
13. Multiple Choice
1 minute
1 pt
C, (graphite) is a good conductor because __________
each carbon atom forms three covalent bonds with other carbon atoms.
there are no delocalised electrons in the giant covalent structure.
there are covalent bonds between the layers.
14. Multiple Choice
1 minute
1 pt
C, (graphite) is a good conductor because __________
there are no covalent bonds between the layers.
each carbon atom forms four covalent bonds with other carbon atoms.
due to the immobile of the electrons.
15. Multiple Choice
1 minute
1 pt
C, (graphite) is a good conductor because __________
there is one non-bonded (or delocalised) electron from each atom.
each carbon atom forms four covalent bonds with other carbon atoms.
there are covalent bonds between the layers.
Atomic forces within the larger molecules are strong.
16. Multiple Choice
1 minute
1 pt
C, (diamond) is an insulator because __________
there are no delocalised electrons in the giant covalent structure.
there is one non-bonded (or delocalised) electron from each atom.
there are no covalent bonds between the layers.
each carbon atom forms three covalent bonds with other carbon atoms.
due to the mobility of the electrons in its outer valence shells.
17. Multiple Choice
1 minute
1 pt
C, (diamond) is an insulator because __________
the carbon atoms form a regular tetrahedral network structure.
there is one non-bonded (or delocalised) electron from each atom.
there are no covalent bonds between the layers.
each carbon atom forms three covalent bonds with other carbon atoms.
due to the mobility of the electrons in its outer valence shells.
18. Multiple Choice
1 minute
1 pt
C, (diamond) is an insulator because __________
there are no free electrons.
there is one non-bonded (or delocalised) electron from each atom.
there are no covalent bonds between the layers.
each carbon atom forms three covalent bonds with other carbon atoms.
due to the mobility of the electrons in its outer valence shells.
19. Multiple Choice
1 minute
1 pt
Choose the correct facts of element from group 14.
Si, Silicon is a semiconductor because it is metalloids / semi metal.
Ge, Germanium is a good conductor because they have delocalised electrons in their giant metallic structures.
Sn, Tin is a semiconductor because it is metalloids / semi metal.
Pb, Lead is a semiconductor because it is metalloids / semi metal.
20. Multiple Choice
1 minute
1 pt
Choose the correct facts of element from group 14.
Ge, Germanium is a semiconductor because it is metalloids / semi metal.
Si, Silicon is a good conductor because they have delocalised electrons in their giant metallic structures.
Sn, Tin is a semiconductor because it is metalloids / semi metal.
Pb, Lead is a semiconductor because it is metalloids / semi metal.
21. Multiple Choice
1 minute
1 pt
Choose the correct facts of element from group 14.
Sn, Tin is a good conductor because they have delocalised electrons in their giant metallic structures.
Ge, Germanium is a good conductor because they have delocalised electrons in their giant metallic structures.
Si, Silicon is a good conductor because they have delocalised electrons in their giant metallic structures.
Pb, Lead is a semiconductor because it is metalloids / semi metal.
22. Multiple Choice
1 minute
1 pt
Choose the correct facts of element from group 14.
Pb, Lead is a good conductor because they have delocalised electrons in their giant metallic structures.
Ge, Germanium is a good conductor because they have delocalised electrons in their giant metallic structures.
Sn, Tin is a semiconductor because it is metalloids / semi metal.
Si, Silicon is a good conductor because they have delocalised electrons in their giant metallic structures.
23. Multiple Choice
1 minute
1 pt
Choose the correct facts of element from group 14.
Simple covalent substances generally have low melting/ boiling points.
Giant covalent substances, such as diamond, contain many simple covalent molecules.
Between each carbon atom in diamond, there are 3 strong covalent bonds.
24. Multiple Choice
1 minute
1 pt
Choose the correct facts of element from group 14.
Giant covalent substances, such as diamond, contain many strong covalent bonds in a 3D lattice structure.
Simple covalent substances generally have high melting/ boiling points.
Between each carbon atom in diamond, there are 3 strong covalent bonds.
Atomic forces within the larger molecules are strong.
25. Multiple Choice
1 minute
1 pt
Choose the correct facts of element from group 14.
Between each carbon atom in diamond, there are 4 strong covalent bonds.
Simple covalent substances generally have high melting/ boiling points.
Giant covalent substances, such as diamond, contain many simple covalent molecules.
The sp3 hybridised in carbon atom, each Carbon atom has one free p orbital that allows to a non metals arbon to conduct electricity field.
26. Multiple Choice
1 minute
1 pt
Why Carbon has more electrical conductivity than Silicone?
Carbon contains more delocalised electrons
Carbon is a non-metal.
Because each carbon atom is joined to four other carbon atoms by strong covalent bonds.
The sp3 hybridised in carbon atom, each Carbon atom has one free p orbital that allows to a non metals arbon to conduct electricity field.
27. Multiple Choice
1 minute
1 pt
Why Carbon has more electrical conductivity than Silicone?
The Silicone is a metalloid which is a semiconductor.
Carbon is a metal.
There are no delocalised electrons in the giant covalent structure.
The sp3 hybridised in carbon atom, each Carbon atom has one free p orbital that allows to a non metals arbon to conduct electricity field.
28. Multiple Choice
1 minute
1 pt
Why Carbon has more electrical conductivity than Silicone?
The sp2 hybridised in carbon atom, each C atom has one free p orbital, overlaps p orbitals forms a p electron cloud above and below the plane (sheet) of carbon atoms.
The carbon atoms form a regular tetrahedral network structure.
There are no free electrons.
Atomic forces within the larger molecules are strong.
29. Multiple Choice
1 minute
1 pt
When down to group 14, what happens to their melting point? (From carbon to stanum is decrease and slightly increase from Sn to plumbum) and why is it so?
The size of atom is increasing, the attractive force between the atom will decrease.
The atomic radius causes the valence electrons to become more delocalised.
The properties of the elements change from non-metallic to metallic.
Atomic forces within the larger molecules are strong.
30. Multiple Choice
1 minute
1 pt
Which element has the highest melting point in the periodic table?
C, carbon
Si, silicon
Ge, germanium
Sn, tin
Pb, lead
31. Multiple Choice
1 minute
1 pt
Which element has the lowest melting point in the group 14?
Sn, tin
Pb, lead
Si, silicon
Ge, germanium
C, carbon
32. Multiple Choice
1 minute
1 pt
Why does carbon have a higher melting point than Sn (tin)?
Carbon has a smaller atomic radius, so it has stronger covalent bonds
The size of atom is larger causes the valence electrons to become more delocalised.
The properties of the elements change from non-metallic to metallic.
Atomic forces within the larger molecules are strong.
33. Multiple Choice
1 minute
1 pt
Why does carbon have a higher melting point than Sn (tin)?
Sn is a metal and due to its larger atomic size (atomic radius), its metallic bond is relatively weak
The size of atom is larger causes the valence electrons to become more delocalised.
The properties of the elements change from non-metallic to metallic.
Atomic forces within the larger molecules are strong.
34. Multiple Choice
1 minute
1 pt
Why does carbon have a higher melting point than Sn (tin)?
The size of atom is larger, the attractive force between the atom weaker.
The properties of the elements change from non-metallic to metallic.
Atomic forces within the larger molecules are strong.
35. Multiple Choice
1 minute
1 pt
How many allotropes of pure carbon?
3
2
1
36. Multiple Choice
1 minute
1 pt
Compare the correct facts of diamond and graphite in terms of structures bonding, electrical conductivity and hardness?
Diamonds: sp3 orbitals arranged in a tetrahedral. Graphite: sp2 hybridised arranged in a plane (sheet).
Diamonds: Conductor, because the delocalised p electrons can move between the planes of the carbon atoms (use as an electrode). Graphite: Insulator, because of all the valence electrons used in bonding.
Diamonds: The soft, slippery is because of the sheet - like structure the layers held together by weak London dispersions forces. Graphite: The hardest substances is because of the 3D network of strong single covalent bonds.
37. Multiple Choice
1 minute
1 pt
Compare the correct facts of diamond and graphite in terms of structures bonding, electrical conductivity and hardness?
Diamonds: Insulator, because of all the valence electrons used in bonding. Graphite: Conductor, because the delocalised p electrons can move between the planes of the carbon atoms (use as an electrode).
Diamonds: sp2 hybridised arranged in a plane (sheet). Graphite: sp3 orbitals arranged in a tetrahedral.
Diamonds: The soft, slippery is because of the sheet - like structure the layers held together by weak London dispersions forces. Graphite: The hardest substances is because of the 3D network of strong single covalent bonds.
38. Multiple Choice
1 minute
1 pt
Compare the correct facts of diamond and graphite in terms of structures bonding, electrical conductivity and hardness?
Diamonds: The hardest substances is because of the 3D network of strong single covalent bonds. Graphite: The soft, slippery is because of the sheet - like structure the layers held together by weak London dispersions forces.
Diamonds: sp2 hybridised arranged in a plane (sheet). Graphite: sp3 orbitals arranged in a tetrahedral.
Diamonds: Conductor, because the delocalised p electrons can move between the planes of the carbon atoms (use as an electrode). Graphite: Insulator, because of all the valence electrons used in bonding.
39. Multiple Choice
1 minute
1 pt
Tetrachloride of group 14, CCl4, SiCl4, GeCl4, SnCl4 and PbCl2. What is the thermal stability when down group 14?
Decreases.
Increases.
Decreases, then increases.
Increases, then decreases,
40. Multiple Choice
1 minute
1 pt
Which one has highest melting point? CH4, SiCl4, SnCl2, SnCl4, PbCl4
SnCl2
CH4
SiCl4
SnCl4
PbCl4
41. Multiple Choice
1 minute
1 pt
Which one has higher melting point? SiCl4, SnCl2. Give the reasons.
SnCl2 is an ionic compounds, ions held together by strong ionic bonds.
SnCl4 molecule are held with the help of strong electronic forces between the opposite charges ion.
SnCl4 is an ionic compound and SnCl2 is a covalent compound.
42. Multiple Choice
1 minute
1 pt
Give reason for each of the following: SnCl2 is a solid while SnCl4 is a liquid at room temperature.
The size of Sn2+ ion is larger than Sn4+ ion.
SnCl2 exist as a liquid because molecule are held together by weak van der Waals forces.
SnCl4 molecule are held with the help of strong electronic forces between the opposite charges ion.
43. Multiple Choice
1 minute
1 pt
Give reason for each of the following: SnCl2 is a solid while SnCl4 is a liquid at room temperature.
SnCl2 is an ionic compound and SnCl4 is a covalent compound.
The size of Sn4+ ion is larger than Sn2+ ion.
SnCl4 molecule are held with the help of strong electronic forces between the opposite charges ion.
44. Multiple Choice
1 minute
1 pt
Give reason for each of the following: SnCl2 is a solid while SnCl4 is a liquid at room temperature.
SnCl2 is solid because molecule are held with the help of strong electronic forces between the opposite charges ion.
The size of Sn4+ ion is larger than Sn2+ ion.
SnCl2 exist as a liquid because molecule are held together by weak van der Waals forces.
45. Multiple Choice
1 minute
1 pt
What is inert pair effect? the tendency of......
electrons in the outermost atomic s orbital to remain unionized in compounds of post-transition metals.
atomic radius causes the valence electrons to become more delocalised.
46. Multiple Choice
1 minute
1 pt
What is inert pair effect? the tendency of......
heavier atoms to form ions with a difference in charge of two.
the delocalised p electrons can move between the planes of the carbon atoms.
47. Multiple Choice
1 minute
1 pt
What is inert pair effect? the tendency of......
electrons remaining paired in valene shell.
the valence electrons used in bonding.
48. Multiple Choice
1 minute
1 pt
What is the reason for inert pair effect?
The inertness of the inner s electrons due to poor shielding.
the valence electrons used in bonding.
49. Multiple Choice
1 minute
1 pt
Why does inert pair effect increase down the group?
The inertness of the inner s electrons due to poor shielding.
the delocalised p electrons can move between the planes of the carbon atoms.
50. Multiple Choice
1 minute
1 pt
Why happens to the inert pair effect when down the group?