| Date | November 2020 | Marks available | 1 | Reference code | 20N.1.sl.TZ0.12 |
| Level | SL | Paper | 1 | Time zone | TZ0 |
| Command term | List and Deduce | Question number | 12 | Adapted from | N/A |
Question
Which series shows the correct order of metallic bond strength from strongest to weakest?
A.
B.
C.
D.
Markscheme
D
Examiners report
A small majority of candidates could identify the relative strength of metallic bonding amongst group 1 and 2 metals.
Syllabus sections
-
18M.2.sl.TZ1.2d.ii:
Outline why solid calcium is a good conductor of electricity.
- 17M.1.sl.TZ1.9: A substance has the following properties: What is the most probable structure of this...
- 17M.1.sl.TZ2.12: Which metal has the strongest metallic bond? A. Li B. Na C. K D. Rb
- 18M.1.hl.TZ1.11: Which metal has the strongest metallic bonding? A. Na B. Mg C. Al D. Ca
-
18M.2.hl.TZ1.2d.ii:
Outline why solid calcium is a good conductor of electricity.
-
22M.2.hl.TZ2.5c:
Describe the bonding in iron, Fe (s).
- 19M.1.hl.TZ1.11: Which combination corresponds to a strong metallic bond?
- 19M.1.hl.TZ2.10: Which combination causes the strength of metallic bonding to increase?
- 19M.1.sl.TZ1.12: Which combination corresponds to a strong metallic bond?
- 19M.1.sl.TZ2.10: Which combination causes the strength of metallic bonding to increase?
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17M.2.sl.TZ1.2d.ii:
Explain why an aluminium-titanium alloy is harder than pure aluminium.
-
17M.2.hl.TZ1.2d.ii:
Suggest why the melting point of vanadium is higher than that of titanium.
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17N.2.sl.TZ0.2b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
-
17M.2.sl.TZ1.2a:
Describe the bonding in metals.
-
17N.2.hl.TZ0.3b:
Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas the melting points of the group 17 elements (F → I) increase down the group.
- 21M.2.hl.TZ2.2b(ii): Describe metallic bonding and how it contributes to electrical conductivity.
- 21M.2.hl.TZ1.1a: Outline why metals, like iron, can conduct electricity.
- 21M.2.hl.TZ1.1d(v): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
- 21M.2.hl.TZ1.1f: Explain why the addition of small amounts of carbon to iron makes the metal harder.
- 21M.2.sl.TZ1.1a: Outline why metals, like iron, can conduct electricity.
- 21M.2.sl.TZ1.1e: Explain why the addition of small amounts of carbon to iron makes the metal harder.
- 20N.2.sl.TZ0.4d(iii): Describe the bonding in metals.
- 20N.3.sl.TZ0.4b(i): Alloying metals changes their properties. Suggest one property of magnesium that could be...
- 20N.2.sl.TZ0.4d(iv): Nickel alloys are used in aircraft gas turbines. Suggest a physical property altered by the...
- 20N.2.hl.TZ0.4d(vi): Nickel alloys are used in aircraft gas turbines. Suggest a physical property altered by the...
- 20N.2.hl.TZ0.4d(v): Describe the bonding in metals.
-
20N.3.hl.TZ0.4c(i):
Alloying metals changes their properties. Suggest one property of magnesium that could be improved by making a magnesium–CNT alloy.
- 21M.2.sl.TZ2.2b(ii): Describe metallic bonding and how it contributes to electrical conductivity.
- 21M.2.sl.TZ1.1c(iv): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
