learning check\n1. draw a simple outline of the periodic table. use shading to identify where the metals and…

learning check\n1. draw a simple outline of the periodic table. use shading to identify where the metals and the non - metals are.\n2. name the group of elements that is not reactive. what feature makes the elements in this group not reactive?\n3. name the element in each pair that is more reactive, and explain how you know.\na) k and na b) f and cl c) na and mg d) s and cl\n4. using figure 2.7 as a guide, sketch the cells for the elements potassium and calcium. your sketch must show the chemical symbol and the electron shells with their electrons.

learning check\n1. draw a simple outline of the periodic table. use shading to identify where the metals and the non - metals are.\n2. name the group of elements that is not reactive. what feature makes the elements in this group not reactive?\n3. name the element in each pair that is more reactive, and explain how you know.\na) k and na b) f and cl c) na and mg d) s and cl\n4. using figure 2.7 as a guide, sketch the cells for the elements potassium and calcium. your sketch must show the chemical symbol and the electron shells with their electrons.

Answer

1.

Brief Explanations:

Draw a rectangular grid representing the periodic - table layout. Shade the left - hand and middle sections for metals and the right - hand section for non - metals.

Answer:

A simple outline of the periodic table with appropriate shading for metals and non - metals as described above.

2.

Brief Explanations:

The noble gases (Group 18) are non - reactive. They have a full outer electron shell, which gives them a stable electron configuration.

Answer:

The group of non - reactive elements is the noble gases (Group 18). Their full outer electron shell makes them non - reactive.

3.

Brief Explanations:

a) Potassium (K) is more reactive than sodium (Na) because as you go down Group 1, the outermost electron is further from the nucleus and easier to lose. b) Fluorine (F) is more reactive than chlorine (Cl) because as you go up Group 17, the atom is smaller and can attract an electron more strongly. c) Sodium (Na) is more reactive than magnesium (Mg) because Na has only one electron in its outer shell and wants to lose it more easily than Mg which has two outer electrons. d) Chlorine (Cl) is more reactive than sulfur (S) because Cl needs one electron to complete its outer shell while S needs two, and Cl has a higher electronegativity.

Answer:

a) K is more reactive. Reason: Outer electron is further from nucleus in K (Group 1 trend). b) F is more reactive. Reason: Smaller atom, stronger electron - attracting ability (Group 17 trend). c) Na is more reactive. Reason: Easier to lose outer electron (1 vs 2 outer electrons). d) Cl is more reactive. Reason: Higher electronegativity, needs 1 electron to complete shell.

4.

Brief Explanations:

Potassium (K) has 19 electrons. Its electron configuration is 2, 8, 8, 1. Draw a circle for the nucleus with 'K' inside, and four electron - shells with 2, 8, 8, 1 electrons respectively. Calcium (Ca) has 20 electrons. Its electron configuration is 2, 8, 8, 2. Draw a circle for the nucleus with 'Ca' inside, and four electron - shells with 2, 8, 8, 2 electrons respectively.

Answer:

For potassium: Nucleus with 'K' inside, 4 electron - shells with 2, 8, 8, 1 electrons. For calcium: Nucleus with 'Ca' inside, 4 electron - shells with 2, 8, 8, 2 electrons.