Analysis and Conclusions:
1.) Define atomic radius
- The atomic radius is used to describe the size of an atom. The atomic radius is the distance from the electron cloud to the nucleus. Because electron cloud is a probability, in order to find the atomic radius, find the distance between the nucleuses of two atoms and divide it by 2.
2.) Use your graphs to describe the trends in atomic radius as you move across the row and down the group
- According to the graph, the atomic radius increase form top to bottom and decreases from left to right. The graphs
3.) Explain the factors that determine these trends in atomic radius
- The atomic radius decreases from left to right because the positive attraction of the electron due to the increasing number of protons. The atomic radius increases from top to bottom because an additional energy level is added each row. Each additional energy level causes the shielding effect to occur. The shielding effect is when the attraction between electrons and the positive nucleus decrease in any atom with the additional energy levels.
4.) How would the trend in ionic radii of period 3 and group 1 compare to the results you observed for atomic radii? Explain.
- The ionic radius is the radius of an atom’s ion. The trends for the ionic radii of period 3 and group 1 depend on the ion’s charge. If the charge is positive, the ionic radius would be less than the atomic radius because an electron is being taken away. If an electron is taken away there will be less electron repulsion, therefore, the ionic radius will be smaller. However, if the atom has a negative charge, then the addition of electrons will cause a shielding effect and electron repulsion, so the ionic radius will be larger than the atomic radius.
5.) Define first ionization energy
- The first ionization energy is the energy required to remove the first electron from gaseous atoms or ions.
6.) Use your graphs to describe the trends in ionization energies as you move across the row and down the group
- According to the graph, as you move down a group the first ionization energy decreases because the valence electrons are farther away from the nucleus and have a weaker attraction to the positive nucleus. Generally, the first ionization increases from left to right from the graph.
7.) Explain the factors that determine these trends in ionization energies. Make sure you explain why the line is not smooth as you move across the row.
- The line is not as smooth as you move across the row because it take more energy to remove an out-shell electron than an inner-shell electron.
8.) How would the trend in electron affinities of the elements in period 3 and group 1 compare to the results you observed for ionization energies? Explain.
- Electron affinities of the elements in period 3 and group 1 are similar to the trends in ionization energies. Electron affinity decreases going down the groups and increases to the right.
9.) What are the characteristics of a metal, a nonmetal, a metalloid, and a noble gas?
- A metal is an element, compound, or alloy that conducts electricity and heat. The physical characteristics of a metal are malleable, ductile, and shiny. Nonmetals are poor conductors of heat and electricity, dull and brittle. Nonmetals also have high electronegativity. Metalloids exhibit characteristics of both metals and nonmetals. They are brittle in the solid state and are relatively good conductors of electricity. They behave as weak nonmetals and have middle ranges of ionization energy and electronegativity values.
10.) Classify the elements in period 3 as metals, metalloids, nonmetals, and noble gases.
- Sodium, Aluminum, and Magnesium are metals. Argon is a noble gas. Chlorine, Sulfur, and Phosphorus are nonmetals and Silicon is a metalloid.
11.) Why are group 1 elements the most active metals and group 17 elements the most active nonmetals.
- The elements in group 1 are the most active metals because they need to lose one valence electron in order to become stable. Group 17 have 7 valence electrons and they need to gain one to fulfill the octet rule.
1.) Create a periodic table to organize these elements based on properties. You may skip spaces
1.) Define atomic radius
- The atomic radius is used to describe the size of an atom. The atomic radius is the distance from the electron cloud to the nucleus. Because electron cloud is a probability, in order to find the atomic radius, find the distance between the nucleuses of two atoms and divide it by 2.
2.) Use your graphs to describe the trends in atomic radius as you move across the row and down the group
- According to the graph, the atomic radius increase form top to bottom and decreases from left to right. The graphs
3.) Explain the factors that determine these trends in atomic radius
- The atomic radius decreases from left to right because the positive attraction of the electron due to the increasing number of protons. The atomic radius increases from top to bottom because an additional energy level is added each row. Each additional energy level causes the shielding effect to occur. The shielding effect is when the attraction between electrons and the positive nucleus decrease in any atom with the additional energy levels.
4.) How would the trend in ionic radii of period 3 and group 1 compare to the results you observed for atomic radii? Explain.
- The ionic radius is the radius of an atom’s ion. The trends for the ionic radii of period 3 and group 1 depend on the ion’s charge. If the charge is positive, the ionic radius would be less than the atomic radius because an electron is being taken away. If an electron is taken away there will be less electron repulsion, therefore, the ionic radius will be smaller. However, if the atom has a negative charge, then the addition of electrons will cause a shielding effect and electron repulsion, so the ionic radius will be larger than the atomic radius.
5.) Define first ionization energy
- The first ionization energy is the energy required to remove the first electron from gaseous atoms or ions.
6.) Use your graphs to describe the trends in ionization energies as you move across the row and down the group
- According to the graph, as you move down a group the first ionization energy decreases because the valence electrons are farther away from the nucleus and have a weaker attraction to the positive nucleus. Generally, the first ionization increases from left to right from the graph.
7.) Explain the factors that determine these trends in ionization energies. Make sure you explain why the line is not smooth as you move across the row.
- The line is not as smooth as you move across the row because it take more energy to remove an out-shell electron than an inner-shell electron.
8.) How would the trend in electron affinities of the elements in period 3 and group 1 compare to the results you observed for ionization energies? Explain.
- Electron affinities of the elements in period 3 and group 1 are similar to the trends in ionization energies. Electron affinity decreases going down the groups and increases to the right.
9.) What are the characteristics of a metal, a nonmetal, a metalloid, and a noble gas?
- A metal is an element, compound, or alloy that conducts electricity and heat. The physical characteristics of a metal are malleable, ductile, and shiny. Nonmetals are poor conductors of heat and electricity, dull and brittle. Nonmetals also have high electronegativity. Metalloids exhibit characteristics of both metals and nonmetals. They are brittle in the solid state and are relatively good conductors of electricity. They behave as weak nonmetals and have middle ranges of ionization energy and electronegativity values.
10.) Classify the elements in period 3 as metals, metalloids, nonmetals, and noble gases.
- Sodium, Aluminum, and Magnesium are metals. Argon is a noble gas. Chlorine, Sulfur, and Phosphorus are nonmetals and Silicon is a metalloid.
11.) Why are group 1 elements the most active metals and group 17 elements the most active nonmetals.
- The elements in group 1 are the most active metals because they need to lose one valence electron in order to become stable. Group 17 have 7 valence electrons and they need to gain one to fulfill the octet rule.
1.) Create a periodic table to organize these elements based on properties. You may skip spaces
1.) Using your periodic table, predict the atomic number of an element with an atomic mass of 11.29 that has nonmetallic properties and is very reactive.
- An element with an atomic radius of 11.29 would have an atomic number of 6 or 7.
2.) Predict the atomic number of an element having an atomic mass of 15.02 that exhibits metallic properties but is softer than lambda and harder than beta
- The atomic number for an element that has an atomic mass of 15.02 would be 8.
3.) Analyze your periodic table for periodic trends, and describe the trends that you identify
- The atomic radius increases from top to bottom and decreases from left to right.
4.) Which of these elements would have the largest atomic radius? The smallest? Which of these elements would have the highest first ionization energy? The lowest?
- Epsilon would have the largest atomic radius because it is the furthest down and would have the most energy levels. Delta would have the smallest radius because it has the fewest energy levels.
- An element with an atomic radius of 11.29 would have an atomic number of 6 or 7.
2.) Predict the atomic number of an element having an atomic mass of 15.02 that exhibits metallic properties but is softer than lambda and harder than beta
- The atomic number for an element that has an atomic mass of 15.02 would be 8.
3.) Analyze your periodic table for periodic trends, and describe the trends that you identify
- The atomic radius increases from top to bottom and decreases from left to right.
4.) Which of these elements would have the largest atomic radius? The smallest? Which of these elements would have the highest first ionization energy? The lowest?
- Epsilon would have the largest atomic radius because it is the furthest down and would have the most energy levels. Delta would have the smallest radius because it has the fewest energy levels.