Which has the larger ionization energy? Sodium (Na), or potassium (K). Why? Which has the larger...
Which has the larger ionization energy? Sodium (Na), or potassium (K). Why?
Which has the larger radius? Sulfur (S), or the sulfide anion (S2-). Why?
If an element has a "large negative" electron affinity number where would it be located on the periodic table?
Homework Answers
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Which has the larger ionization energy? Sodium (Na), or
potassium (K). Why?
Which has the larger...
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...
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers...
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers to energy required to remove an outer electron from an isolated atom. The energy tends to be less for elements with weaker attractions to the nucleus or higher initial energy levels. The general trend is for lower energy for elements lower in columns and higher energy from left to right across rows of the periodic table. There are some notable exceptions. Explain why: 2....
7. Which element has the following electron configurations? lon: [Ar]3d10 lon (-1 charge): [Kr]5s4d105p6 8. Write t...
7. Which element has the following electron configurations? lon: [Ar]3d10 lon (-1 charge): [Kr]5s4d105p6 8. Write the following in order of increasing size As O Br Br Na Rb Te²- F- 02- 9. Arrange these elements in order of decreasing first ionization energy: CI, S, Sn, Pb 10. Choose the element with a more negative (exothermic) electron affinity in each pair: K or Cs Si or P Ga or Br Mg or s 11. a) Which has a higher ionization...
Also, why is second IE Mg less than second IE Al? Why 3rd IE Mg larger...
Also, why is second IE Mg less than second IE Al? Why 3rd IE
Mg larger than 3rd IE Al? If you could explain IE and EA very
simply thatd be great!
Match the element to the description. Your choices are: Na, AI, P, CI, Ar (you will use only four of these!) a. -An unreactive gas with a large ionization energy and no measurable electron affinity. b. A very reactive solid that forms a basic oxide. It has a...
Element Na First Ionization Energy (J/mol) 4.95 x 105 4.19 x 105 K 6. The first...
Element Na First Ionization Energy (J/mol) 4.95 x 105 4.19 x 105 K 6. The first ionization energies for Na and K are given in the table above. a. Write the complete electron configuration for Na. b. Based on principles of atomic structure, explain why the first ionization energy of K is lower than the first ionization energy of Na. c. Which ionic solid would have the greatest melting point, NaCl or KCI? Justify your answer in terms of lattice...
Which of the following statements is true? i fixed the question a. Both ionization energy and...
Which of the following statements is true? i fixed the question a. Both ionization energy and electron affinity increase as you move across a row of the periodic table. b. Both metallic character and electron affinity increase as you move across a row of the periodic table. c. Ionization energy increases and electron affinity decreases as you move across a row of the periodic table. d. Metallic character increases and ionization energy decreases as you move across a row of...
Predict which element in each of the following pairs has the larger ionization energy K or...
Predict which element in each of the following pairs has the larger ionization energy K or Br S or Te Ga or Se Ne or Sr
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).
explanation needed thank u . Which element has a larger SECOND ionization energy, Ca or K?...
explanation needed thank u
. Which element has a larger SECOND ionization energy, Ca or K? Explain.
Organic chemistry b. Which atom has the higher first ionization potential and why? (F or S)...
Organic chemistry
b. Which atom has the higher first ionization potential and why? (F or S) c. Which neutral atom has the larger atomic radius and why? (S or CI) d. Which anion has the larger radius and why? (Br'l or Se) e. Which cation has the larger radius and why? (Na* or Mg2)
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...
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers to energy required to remove an outer electron from an isolated atom. The energy tends to be less for elements with weaker attractions to the nucleus or higher initial energy levels. The general trend is for lower energy for elements lower in columns and higher energy from left to right across rows of the periodic table. There are some notable exceptions. Explain why: 2....
7. Which element has the following electron configurations? lon: [Ar]3d10 lon (-1 charge): [Kr]5s4d105p6 8. Write the following in order of increasing size As O Br Br Na Rb Te²- F- 02- 9. Arrange these elements in order of decreasing first ionization energy: CI, S, Sn, Pb 10. Choose the element with a more negative (exothermic) electron affinity in each pair: K or Cs Si or P Ga or Br Mg or s 11. a) Which has a higher ionization...
Also, why is second IE Mg less than second IE Al? Why 3rd IE
Mg larger than 3rd IE Al? If you could explain IE and EA very
simply thatd be great!
Match the element to the description. Your choices are: Na, AI, P, CI, Ar (you will use only four of these!) a. -An unreactive gas with a large ionization energy and no measurable electron affinity. b. A very reactive solid that forms a basic oxide. It has a...
Element Na First Ionization Energy (J/mol) 4.95 x 105 4.19 x 105 K 6. The first ionization energies for Na and K are given in the table above. a. Write the complete electron configuration for Na. b. Based on principles of atomic structure, explain why the first ionization energy of K is lower than the first ionization energy of Na. c. Which ionic solid would have the greatest melting point, NaCl or KCI? Justify your answer in terms of lattice...
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).
explanation needed thank u
. Which element has a larger SECOND ionization energy, Ca or K? Explain.
Organic chemistry
b. Which atom has the higher first ionization potential and why? (F or S) c. Which neutral atom has the larger atomic radius and why? (S or CI) d. Which anion has the larger radius and why? (Br'l or Se) e. Which cation has the larger radius and why? (Na* or Mg2)
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