What is the trend for …. When you go across the period? Down a family? For...
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What is the trend for …. When you go across the period? Down a family?
For each trend, explain in your own words what it means and/or why it is.
a) atomic size?
b) ionization energy?
c) electron affinity?
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Which should be larger according to the general trend? Explain.
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Li, Na?
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K or K+?
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Cl or Cl-?
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P or S?
Homework Answers
based on the periodic properties the trends and the
values as follows
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What is the trend for …. When you go across the period?
Down a family?
For...
The maximum number of electrons in n=3 4d One orbital by the name of 3p Shell...
The maximum number of electrons in n=3 4d One orbital by the name of 3p Shell 4 Subshell g Write an chemical equation that goes with… a) heat of combustion of Mg. b) heat of formation of PBr3(s) c) First ionization energy of Na. d) second electron affinity of oxygen. What is the trend for …. When you go across the period? Down a family? For each trend, explain in your own words what it means and/or why it is. a)...
1. Write electron configuration for …. DO NOT use the core notation. Write out the last...
1. Write electron configuration for …. DO NOT use the core notation. Write out the last one so it would match the Box diagram. ( for example, write ….2p1,1,0 instead of 2p2). a) Sn b) Ba c)Nb d) Mg 2. Write electron configuration for …. Use the core notation. Write out the last one so it would match the Box diagram. ( for example, write ….2p1,1,0 instead of 2p2). a) Sn a) Zr Co Kr As 3. How many families...
no need for explanation and will rate immediately, thank you. 1. Determine the trend for each...
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need for explanation and will rate immediately,
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1. Determine the trend for each property (i.e. whether it increases or decreases): Across a row of the Down a column in the PT PT? Size Ionization energy Electron affinity 1. Within a given row, which Group of elements has the greatest atomic size? (a) The alkali metals (b) The halogens (c) The noble gases (d) Another Group (give the Group number using the IUPAC system) 2. Within a given...
What is the general trend in ionization energy across a row on the periodic table? Using...
What is the general trend in ionization energy across a row on the periodic table? Using a ground state electron configuration as your basis of comparison, explain Why the ionization energy of boron is less than that of beryllium Why the ionization energy of oxygen is less than that of nitrogen
6 a, b and c 7 a, b and c will rate thanks. ople Tab Window...
6
a, b and c
7 a, b and c
will rate thanks.
ople Tab Window Help 2247% s for Chemistry X Chad's Prep -- FREE Chem x + cute/content/file?cmd=view&content_id=_4296552_1&course_id=_123382_1 6. (a) Write the equation (half-reaction) representing the ionization energy of Li. From what orbital is the electron removed in this process? (b) Write the equation representing the ionization energy of Na. From what orbital is the electron removed in this process? (c). Comparing your answers in (a) and (b),...
34. Explain the general trend for atomic radius going across a period; to the right. 35....
34. Explain the general trend for atomic radius going across a period; to the right. 35. Explain the general trend in atomic radius going down a group.
Report: Periodic Properties Valence Electrons +Electron Configurations 1. Give the condensed electron configuratio...
Report: Periodic Properties Valence Electrons +Electron Configurations 1. Give the condensed electron configuration for the following elements. Rb d. I a. b. С e. Ca c. Si f. Pb Give the number of valence electrons for each element. 2. d. Br a. Al b. Rb c. Ar 3. Across a period of the periodic table (left to right), valence electrons... Circle the correct choice: (increase / remain the same / decrease) Down a family of the periodic table (top to...
8-7 Why is the first ionization energy for phosphorous higher than the first ionization energy for...
8-7 Why is the first ionization energy for phosphorous higher than the first ionization energy for sulfur even though the general trend in the periodic table is to have the ionization energy increase as you go from left to right on the table. 8-8 The three most common oxidation states for Fe are +2, +3 and +6 what are the most likely electronic configurations for these three ions? 8-9 Why do transition metals have magnetic properties? 8-10 Just looking at...
Question 9 Which of these statements is false? An anion is always larger than its parent...
Question 9 Which of these statements is false? An anion is always larger than its parent neutral atom. The first electron affinity is always a large negative value. First ionization energy decreases in going down a column (group). Second ionization energies are always larger than first ionization energies. Atomic size decreases in going from left to right across a row (period).
Ionization energy Ionization Energy is the energy required to remove an electron from an atom or...
Ionization energy Ionization Energy is the energy required to remove an electron from an atom or ion in the gaseous state. The ionization energy is always positive because it takes energy to remove and electron. 1) Using the figure on the left, which elements have the highest first ionization energies? 2) Does this make sense as to why they have high Ionization energy? ell tentation energi 3) Which elements have the lowest first ionization energies? 4 Does this make sense...
no
need for explanation and will rate immediately,
thank you.
1. Determine the trend for each property (i.e. whether it increases or decreases): Across a row of the Down a column in the PT PT? Size Ionization energy Electron affinity 1. Within a given row, which Group of elements has the greatest atomic size? (a) The alkali metals (b) The halogens (c) The noble gases (d) Another Group (give the Group number using the IUPAC system) 2. Within a given...
What is the general trend in ionization energy across a row on the periodic table? Using a ground state electron configuration as your basis of comparison, explain Why the ionization energy of boron is less than that of beryllium Why the ionization energy of oxygen is less than that of nitrogen
6
a, b and c
7 a, b and c
will rate thanks.
ople Tab Window Help 2247% s for Chemistry X Chad's Prep -- FREE Chem x + cute/content/file?cmd=view&content_id=_4296552_1&course_id=_123382_1 6. (a) Write the equation (half-reaction) representing the ionization energy of Li. From what orbital is the electron removed in this process? (b) Write the equation representing the ionization energy of Na. From what orbital is the electron removed in this process? (c). Comparing your answers in (a) and (b),...
34. Explain the general trend for atomic radius going across a period; to the right. 35. Explain the general trend in atomic radius going down a group.
Report: Periodic Properties Valence Electrons +Electron Configurations 1. Give the condensed electron configuration for the following elements. Rb d. I a. b. С e. Ca c. Si f. Pb Give the number of valence electrons for each element. 2. d. Br a. Al b. Rb c. Ar 3. Across a period of the periodic table (left to right), valence electrons... Circle the correct choice: (increase / remain the same / decrease) Down a family of the periodic table (top to...
8-7 Why is the first ionization energy for phosphorous higher than the first ionization energy for sulfur even though the general trend in the periodic table is to have the ionization energy increase as you go from left to right on the table. 8-8 The three most common oxidation states for Fe are +2, +3 and +6 what are the most likely electronic configurations for these three ions? 8-9 Why do transition metals have magnetic properties? 8-10 Just looking at...
Question 9 Which of these statements is false? An anion is always larger than its parent neutral atom. The first electron affinity is always a large negative value. First ionization energy decreases in going down a column (group). Second ionization energies are always larger than first ionization energies. Atomic size decreases in going from left to right across a row (period).
Ionization energy Ionization Energy is the energy required to remove an electron from an atom or ion in the gaseous state. The ionization energy is always positive because it takes energy to remove and electron. 1) Using the figure on the left, which elements have the highest first ionization energies? 2) Does this make sense as to why they have high Ionization energy? ell tentation energi 3) Which elements have the lowest first ionization energies? 4 Does this make sense...
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