from xv.chemistry.inorganic import ElementGroupManager

ke = ElementGroupManager()
ke

2637928871392@ElementGroupManager

Details of elements


Minimum Grade: 6
Maximum Grade: 12


Examples
--------
ke = ElementGroupManager()
ke

ke.printProblemTypes()

ke.getRandomProblem()
ke.getRandomProblem(problem_type = 0)
...

ke.printProblem()
ke.printAnswer()
ke.printSolution()


doc_style: xv_doc

ke.printProblemTypes()

0. _problem_group_elements
1. _problem_group_1_elements_TEMP

from IPython.display import HTML
n = len(ke._problemTemplates)
max_loop = 1
for j in range(0, max_loop):
    for i in range(n):
        problem_type = i
        display(HTML(f"<h2>problem_type: {problem_type}/{n-1} (loop {j}/{max_loop-1})</h2>"))
        ke.getRandomProblem(problem_type = problem_type, verbose = True)
        display(ke.printProblem())

        display(HTML(f"<h6>Answer:</h6>"))
        display(ke.printAnswer())

        display(HTML(f"<h6>Solution:</h6>"))
        display(ke.printSolution())
        pass

problem_type: 0/1 (loop 0/0)

Problem Template: _problem_group_elements

Properties of the elements of group: 15.

Answer:

Electronic Configuration:

Name (Symbol) Atomic Number: Electronic configuration
Nitrogen (N) 7: 1s2 2s2 2p3
Phosphorus (P) 15: 1s2 2s2 2p6 3s2 3p3
Arsenic (As) 33: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3
Antimony (Sb) 51: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10 5s2 5p3
Bismuth (Bi) 83: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 4f14 5d10 6s2 6p3
Moscovium (Mc) 115: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 5f14 6d10 7s2 7p3

State at normal temperature and pressure:

gases: Nitrogen
solids: Antimony, Phosphorus, Arsenic, Bismuth, Moscovium

General properties of the elements of group 15:
Not implemented group_id: 15

Solution:

Electronic Configuration:

Name (Symbol) Atomic Number: Electronic configuration
Nitrogen (N) 7: 1s2 2s2 2p3
Phosphorus (P) 15: 1s2 2s2 2p6 3s2 3p3
Arsenic (As) 33: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3
Antimony (Sb) 51: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10 5s2 5p3
Bismuth (Bi) 83: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 4f14 5d10 6s2 6p3
Moscovium (Mc) 115: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 5f14 6d10 7s2 7p3

State at normal temperature and pressure:

gases: Nitrogen
solids: Antimony, Phosphorus, Arsenic, Bismuth, Moscovium

General properties of the elements of group 15:
Not implemented group_id: 15

problem_type: 1/1 (loop 0/0)

Problem Template: _problem_group_1_elements_TEMP

Properties of the elements of group: 1.

Answer:

Name (Symbol) Atomic Number: Electronic configuration

Hydrogen (H) 1: 1s1

Lithium (Li) 3: 1s2 2s1

Sodium (Na) 11: 1s2 2s2 2p6 3s1

Potassium (K) 19: 1s2 2s2 2p6 3s2 3p6 4s1

Rubidium (Rb) 37: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1

Cesium (Cs) 55: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s1

Francium (Fr) 87: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s1

General properties of the elements of group 1:

1. They are called alkali metals.
   They are readly give up one electron and thus are alkaline in nature.
   When reacting to water, they form Na+ and OH- ions, the latter in alkaline.
2. The elements are soft and can be cut with a knife.
   
   All the metals cyrstallize with body centered cubic (BCC) lattice, i.e., coordination number is eight. This structure is adopted due to large atomic radius.
   
   It is not the closest packed structure.
   
   As there is only one valence electron per atom, the binding energy in the metal lattice is relatively weak. The metals are, thus, very soft and have low melting points. (A Na — K alloy with 77.2% ...
   
   BCC 3D model
   https://sketchfab.com/3d-models/bcc-84706d2f637542c99e29daa4e40d761c
   https://www.chemtube3d.com/_bccfinal/
   https://www.ibiblio.org/e-notes/Cryst/Cryst.htm
   https://www.ibiblio.org/e-notes/Cryst/BCC.html
   https://en.wikipedia.org/wiki/Periodic_table_(crystal_structure)
   https://opentextbc.ca/chemistry/chapter/10-6-lattice-structures-in-crystalline-solids/
   http://wwwchem.uwimona.edu.jm/courses/CHEM1902/IC10K_MG_struct_elementsAME.html
3. The elements have relatively low melting points.
4. The elements have low densities.
   The first three elements Lithium, Sodium and Potassium) are so light that they can float on water.
5. The elements have relatively low melting points.
6. Atoms of group 1 elements all have one electron in their outer shell. This means that the alkali metals all have similar chemical properties.
7. Reaction with moist air
   Group 1 elements react with moist air. They are stored in oil to stop air and water vapour coming into contact with them. Moist air reacts with potassium to form potassium oxide. This creates a layer over the surface of the metal.
8. Reactions with water
   The alkali metals react with water to produce a metal hydroxide and hydrogen. For example, sodium reacts with water:
   sodium + water → sodium hydroxide + hydrogen
   2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
   
   Lithium, Li: Fizzes steadily, and slowly becomes smaller until it has all reacted
   Sodium, Na: Melts to form a ball, fizzes rapidly, and quickly becomes smaller until it disappears
   Potassium, K: Quickly melts to form a ball, burns violently with sparks and a lilac flame, and reacts rapidly, often with a small explosion
9. Sodium hydroxide is an alkali. It is a base that dissolves in water to form an alkaline solution. This solution:
   has a pH greater than 7
   turns universal indicator solution blue or purple
10. Reaction with chlorine
    The group 1 metals all react with chlorine to produce chlorides. The chlorides are all white solids at room temperature, and dissolve in water to make a neutral solution.
    Sodium + chlorine → sodium chloride
    2Na(s) + Cl2(g) → 2NaCl(s)
    The reactions get more vigorous going down the group.
11. Alkali metals are good conductors of heat and electricity.
12. Alkali metals are good reducing agents because the single valence electron in the atom of each alkali metal can be easily released to achieve a stable electron arrangement of a noble gas (good electron donor).
13. Electropositivity of an element is a measurement of the ability of an atom to donate electrons to form a positive ion.
    Alkali metals are very electropositive.
    This is because the atom of each alkali metal can release its single valence electron easily to form a positive ion.
14. Solubility of the salts of alkali metals
    Carbonate, nitrate, chloride, sulphate, bromide and iodide salts of alkali metals are white solids.
    These salts are soluble in water. They dissolve in water to form colourless solutions.
15. Safety precautions in handling Group 1 elements
    
    Alkali metals are very reactive.
    Alkali metals, when exposed, can react with oxygen and water vapour in the air.
    Hence, alkali metals such as lithium, sodium and potassium must be kept in paraffin oil, whereas rubidium and caesium are stored in sealed glass tubes. This is to prevent them from reacting with oxygen and water vapour in the air.
    The following safety precautions must be taken when handling alkali metals.
    Avoid holding the highly reactive alkali metals with your bare hands.
    Wear safety goggles and gloves during an experiment.
16. The alkali metals are so reactive that they are generally found in nature combined with other elements.

Solution:

Name (Symbol) Atomic Number: Electronic configuration

Hydrogen (H) 1: 1s1

Lithium (Li) 3: 1s2 2s1

Sodium (Na) 11: 1s2 2s2 2p6 3s1

Potassium (K) 19: 1s2 2s2 2p6 3s2 3p6 4s1

Rubidium (Rb) 37: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1

Cesium (Cs) 55: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s1

Francium (Fr) 87: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s1

General properties of the elements of group 1:

1. They are called alkali metals.
   They are readly give up one electron and thus are alkaline in nature.
   When reacting to water, they form Na+ and OH- ions, the latter in alkaline.
2. The elements are soft and can be cut with a knife.
   
   All the metals cyrstallize with body centered cubic (BCC) lattice, i.e., coordination number is eight. This structure is adopted due to large atomic radius.
   
   It is not the closest packed structure.
   
   As there is only one valence electron per atom, the binding energy in the metal lattice is relatively weak. The metals are, thus, very soft and have low melting points. (A Na — K alloy with 77.2% ...
   
   BCC 3D model
   https://sketchfab.com/3d-models/bcc-84706d2f637542c99e29daa4e40d761c
   https://www.chemtube3d.com/_bccfinal/
   https://www.ibiblio.org/e-notes/Cryst/Cryst.htm
   https://www.ibiblio.org/e-notes/Cryst/BCC.html
   https://en.wikipedia.org/wiki/Periodic_table_(crystal_structure)
   https://opentextbc.ca/chemistry/chapter/10-6-lattice-structures-in-crystalline-solids/
   http://wwwchem.uwimona.edu.jm/courses/CHEM1902/IC10K_MG_struct_elementsAME.html
3. The elements have relatively low melting points.
4. The elements have low densities.
   The first three elements Lithium, Sodium and Potassium) are so light that they can float on water.
5. The elements have relatively low melting points.
6. Atoms of group 1 elements all have one electron in their outer shell. This means that the alkali metals all have similar chemical properties.
7. Reaction with moist air
   Group 1 elements react with moist air. They are stored in oil to stop air and water vapour coming into contact with them. Moist air reacts with potassium to form potassium oxide. This creates a layer over the surface of the metal.
8. Reactions with water
   The alkali metals react with water to produce a metal hydroxide and hydrogen. For example, sodium reacts with water:
   sodium + water → sodium hydroxide + hydrogen
   2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
   
   Lithium, Li: Fizzes steadily, and slowly becomes smaller until it has all reacted
   Sodium, Na: Melts to form a ball, fizzes rapidly, and quickly becomes smaller until it disappears
   Potassium, K: Quickly melts to form a ball, burns violently with sparks and a lilac flame, and reacts rapidly, often with a small explosion
9. Sodium hydroxide is an alkali. It is a base that dissolves in water to form an alkaline solution. This solution:
   has a pH greater than 7
   turns universal indicator solution blue or purple
10. Reaction with chlorine
    The group 1 metals all react with chlorine to produce chlorides. The chlorides are all white solids at room temperature, and dissolve in water to make a neutral solution.
    Sodium + chlorine → sodium chloride
    2Na(s) + Cl2(g) → 2NaCl(s)
    The reactions get more vigorous going down the group.
11. Alkali metals are good conductors of heat and electricity.
12. Alkali metals are good reducing agents because the single valence electron in the atom of each alkali metal can be easily released to achieve a stable electron arrangement of a noble gas (good electron donor).
13. Electropositivity of an element is a measurement of the ability of an atom to donate electrons to form a positive ion.
    Alkali metals are very electropositive.
    This is because the atom of each alkali metal can release its single valence electron easily to form a positive ion.
14. Solubility of the salts of alkali metals
    Carbonate, nitrate, chloride, sulphate, bromide and iodide salts of alkali metals are white solids.
    These salts are soluble in water. They dissolve in water to form colourless solutions.
15. Safety precautions in handling Group 1 elements
    
    Alkali metals are very reactive.
    Alkali metals, when exposed, can react with oxygen and water vapour in the air.
    Hence, alkali metals such as lithium, sodium and potassium must be kept in paraffin oil, whereas rubidium and caesium are stored in sealed glass tubes. This is to prevent them from reacting with oxygen and water vapour in the air.
    The following safety precautions must be taken when handling alkali metals.
    Avoid holding the highly reactive alkali metals with your bare hands.
    Wear safety goggles and gloves during an experiment.
16. The alkali metals are so reactive that they are generally found in nature combined with other elements.