Question

1. a) What is a general trend in ionization energy going across a period to the...

1. a) What is a general trend in ionization energy going across a period to the right? (across the periodic table to the right)

b) Give one example of when this trend is not followed

c) Fully explain your answer to part b

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The general trend for the first ionization energy (energy necessary to remove an electron from an...
The general trend for the first ionization energy (energy necessary to remove an electron from an atom) for Representative elements is as follows: a. increases across the table and from top to bottom b. decreases across the table and from the top to bottom c. increases across the table and decreases fro top to bottom d. decreases across the table and increases from top to bottom
In general, ionization energies increase across a period from left to right. Explain why the second...
In general, ionization energies increase across a period from left to right. Explain why the second ionization energy of Cr (1592 kj/mol) is higher, not lower, than that of Mn (1509 kj/mol). (Hint: what is the electron configuration of Cr?)
1. Explain atomic size, ionization potential, electronegativity and the general periodic trend for each of these...
1. Explain atomic size, ionization potential, electronegativity and the general periodic trend for each of these properties. Arrange the following atoms: O, Se, C, Si, F in order of increasing atomic radius, in order of increasing electronegativity and in order of increasing ionization energy. Explain how you developed your list and explain the similarities or differences between the lists. 2.The successive ionization energies for boron are 801, 2430, 3670, 25,000, and 32,800 kJ/mole. Why does boron have a fairly low...
(b) Based on your knowledge of the periodic trend in first ionization energy, place the following...
(b) Based on your knowledge of the periodic trend in first ionization energy, place the following in order of INCREASING first ionization energy such that 1 is the element with the lowest predicted first ionization energy and 5 is the element with the highest predicted first ionization energy. 1 2 3 4 5  Zn 1 2 3 4 5  Sr 1 2 3 4 5  N 1 2 3 4 5  Ca 1 2 3 4 5  Ti Incorrect. Tries 1/3 Previous Tries (c) Based...
How much heat would it take to convert 60.0 g ice at 0.00˚C into liquid water...
How much heat would it take to convert 60.0 g ice at 0.00˚C into liquid water at 20.0˚C? The trend in polarizability from left to right across a period in the Periodic Table is due to … a. decreasing electronegativity. b. decreasing ionization energy. c. increasing mass. d. decreasing atomic size.
Which of the following statements is/are correct? 1. For any element, the second ionization energy is...
Which of the following statements is/are correct? 1. For any element, the second ionization energy is larger than the first ionization energy. 2. Ionization energy is a positive value for all elements. 3. Ionization energy increases down a group of the periodic table. No information in our books and professor can't explain how it works, please help.
what additional patterns can you find in the ionization energy for the third period? consider all...
what additional patterns can you find in the ionization energy for the third period? consider all patterns, including where you have the largest increase. give your rational
Briefly define the following terms, describe the periodic trends, and the reason each trend is what...
Briefly define the following terms, describe the periodic trends, and the reason each trend is what it is. a. Electronegativity b. Ionization energy c. Electron affinity d. Atomic radius
1. Based on shielding explain why S2- is larger than S 2. O2- , F- ,...
1. Based on shielding explain why S2- is larger than S 2. O2- , F- , Ne, Na+ and Mg2+ are isoelectronic since they have the same number of electrons. Order them from largest to smallest in radius. Explain your reasoning. 3. In general, how do the following values change as one proceeds left to right on the periodic table: a. Atomic radii b. Ionization energy c. Electron affinity d. Metallic character 4. Write the following chemical equations: a. Reaction...
a)What is the ionization energy (in kJ/mol) for the one-electron species, He+1 ? b)What is the...
a)What is the ionization energy (in kJ/mol) for the one-electron species, He+1 ? b)What is the ionization energy (in kJ/mol) for the one-electron species, P+14 ?