QUIZ
Group 14 Chemistry
3 days ago by
51 questions
Q. What is the first element in group 14?
answer choices
C, carbon
Si, silicon
Ge, germanium
Sn, tin
Pb, lead
Q. What is the second element in group 14?
answer choices
Si, silicon
Ge, germanium
Sn, tin
Pb, lead
C, carbon
Q. What is the third element in group 14?
answer choices
Ge, germanium
Sn, tin
Pb, lead
C, carbon
Si, silicon
Q. What is the fourth element in group 14?
answer choices
Sn, tin
Pb, lead
Si, silicon
Ge, germanium
C, carbon
Q. What is the fifth element in group 14?
answer choices
Pb, lead
C, carbon
Si, silicon
Ge, germanium
Sn, tin
Q. What is the type of bond that is related to group 14 elements’ melting points?
answer choices
Carbon is a non-metal
Silicon and germanium are metals
Tin and Lead are metalloids
Q. What is the type of bond that is related to group 14 elements’ melting points?
answer choices
Silicon and germanium are metalloids
Carbon is a metal
Tin and Lead are metalloids
Q. What is the type of bond that is related to group 14 elements’ melting points?
answer choices
Tin and Lead are metals
Silicon and germanium are non-metals
Carbon is a metalloids
Q. Change in electrical conductivity when going down group 14 is _________.
answer choices
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.
Q. Change in electrical conductivity when going down group 14 is _________.
answer choices
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.
Q. Change in electrical conductivity when going down group 14 is _________.
answer choices
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.
Q. C, (graphite) is a good conductor because __________
answer choices
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.
Q. C, (graphite) is a good conductor because __________
answer choices
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.
Q. C, (graphite) is a good conductor because __________
answer choices
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.
Q. C, (graphite) is a good conductor because __________
answer choices
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.
Q. C, (diamond) is an insulator because __________
answer choices
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.
Q. C, (diamond) is an insulator because __________
answer choices
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.
Q. C, (diamond) is an insulator because __________
answer choices
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.
Q. Choose the correct facts of element from group 14.
answer choices
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.
Q. Choose the correct facts of element from group 14.
answer choices
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.
Q. Choose the correct facts of element from group 14.
answer choices
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.
Q. Choose the correct facts of element from group 14.
answer choices
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.
Q. Choose the correct facts of element from group 14.
answer choices
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.
Q. Choose the correct facts of element from group 14.
answer choices
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.
Q. Choose the correct facts of element from group 14.
answer choices
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.
Q. Why Carbon has more electrical conductivity than Silicone?
answer choices
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.
Q. Why Carbon has more electrical conductivity than Silicone?
answer choices
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.
Q. Why Carbon has more electrical conductivity than Silicone?
answer choices
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.
Q. 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?
answer choices
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.
Q. Which element has the highest melting point in the periodic table?
answer choices
C, carbon
Si, silicon
Ge, germanium
Sn, tin
Pb, lead
Q. Which element has the lowest melting point in the group 14?
answer choices
Sn, tin
Pb, lead
Si, silicon
Ge, germanium
C, carbon
Q. Why does carbon have a higher melting point than Sn (tin)?
answer choices
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.
Q. Why does carbon have a higher melting point than Sn (tin)?
answer choices
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.
Q. Why does carbon have a higher melting point than Sn (tin)?
answer choices
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.
Q.

How many allotropes of pure carbon?

answer choices

3

2

1

Q. Compare the correct facts of diamond and graphite in terms of structures bonding, electrical conductivity and hardness?
answer choices
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.
Q. Compare the correct facts of diamond and graphite in terms of structures bonding, electrical conductivity and hardness?
answer choices
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.
Q. Compare the correct facts of diamond and graphite in terms of structures bonding, electrical conductivity and hardness?
answer choices
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.
Q. Tetrachloride of group 14, CCl4, SiCl4, GeCl4, SnCl4 and PbCl2. What is the thermal stability when down group 14?
answer choices
Decreases.
Increases.
Decreases, then increases.
Increases, then decreases,
Q. Which one has highest melting point? CH4, SiCl4, SnCl2, SnCl4, PbCl4
answer choices
SnCl2
CH4
SiCl4
SnCl4
PbCl4
Q. Which one has higher melting point? SiCl4, SnCl2. Give the reasons.
answer choices
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.
Q. Give reason for each of the following: SnCl2 ​ is a solid while SnCl4 ​ is a liquid at room temperature.
answer choices
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.
Q. Give reason for each of the following: SnCl2 ​ is a solid while SnCl4 ​ is a liquid at room temperature.
answer choices
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.
Q. Give reason for each of the following: SnCl2 ​ is a solid while SnCl4 ​ is a liquid at room temperature.
answer choices
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.
Q. What is inert pair effect? the tendency of......
answer choices
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.
Q. What is inert pair effect? the tendency of......
answer choices
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.
Q. What is inert pair effect? the tendency of......
answer choices
electrons remaining paired in valene shell.
the valence electrons used in bonding.
Q. What is the reason for inert pair effect?
answer choices
The inertness of the inner s electrons due to poor shielding.
the valence electrons used in bonding.
Q. Why does inert pair effect increase down the group?
answer choices
The inertness of the inner s electrons due to poor shielding.
the delocalised p electrons can move between the planes of the carbon atoms.
Q. Why happens to the inert pair effect when down the group?
answer choices
increase
decrease
Q. What is the best way to prepare CCl4?
answer choices
Heat carbon in a flow of dry Cl2 gas.
Heat carbon in a flow of wet Cl2 gas.
Quizzes you may like
15 Qs
Chemical Bonding
10.3k plays
20 Qs
Bonding
8.4k plays
20 Qs
Bond... Covalent Bond
2.8k plays
Chemistry
9 Qs
Types of Solids
493 plays
10 Qs
Types of Bonds
338 plays
Chemistry
13 Qs
Polymers
101 plays
20 Qs
Chemical Bonds
39 plays
20 Qs
Ionic or Covalent Bond?
257 plays
Why show ads?
Report Ad