Homework Answers
explanation:
1) As atomic number is 33. so number of protons are 33. in Br atomic number is 35 so number of protons 35.
number of protons increases nucleous charge also increases so that atomic size decreases
2) metals ionization energy is very low they can readily loose electron . non metals have high ionization energy so they gain electrons
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D Question 10 Why is Bra smaller atom than As? Br is actually larger than As...
If S^2- larger or smaller than Cl- a. these two ions have the same size b/c...
If S^2- larger or smaller than Cl- a. these two ions have the same size b/c they have the same number of electron b. s^2- is larger b/c it has fewer protons than cl- c. s^2- is larger b/c it exhibits greater electron repulsion d. cl- is larger b/c it has higher mass than s2-
Question 4 (1 point) Do you predict 52- or Ca2+ to have a smaller ionic radius?...
Question 4 (1 point) Do you predict 52- or Ca2+ to have a smaller ionic radius? Why? Ca2+ is smaller because it has only two valence electrons whereas S2- has six. OCa2+ is smaller because its nucleus has a larger positive charge which exerts a stronger force than the nucleus of S2- on the same number of electrons. Os2- is smaller because it contains fewer electrons than Ca2+ and therefore has a smaller electron cloud. OS2- is smaller because it...
Question 10 4 pts Which of the following explanations best explains, from first principles, the fact...
Question 10 4 pts Which of the following explanations best explains, from first principles, the fact that boron has a lower first ionization energy than beryllium? 0 Beryllium has more core electrons than boron. 0 Boron is more boring and hence it will be easier to remove the bored electrons from the shell. Electrons are more closely bound in beryllium because God invented the Octet Rule, such that beryllium is closer to an octet than boron. 0 In beryllium, an...
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...
a) Why is the Li+ radius so much smaller than the radius of the neutral Li...
a) Why is the Li+ radius so much smaller than the radius of the neutral Li atom? b) Why is the F- radius so much larger than the neutral F atom? b) Which transition involves the emission of less energy in the H atom, an electron moving from n=4 to n=3 or an electron moving from n=3 to n=2?
Help with explanation if possible. Nae Section -Date Now let's look at chlorine A chlorine atom...
Help with explanation if possible.
Nae Section -Date Now let's look at chlorine A chlorine atom has how many protons Therefore, we know that a chlorine atom has how many electrons? How many electrons will go in the first shell? How many in the second shell? Nucleus How many in the third? Draw this in Figure 2.2 We know that a chlorine atom requires eight electrons in its valence shell to become stable. Will it be easier for chlorine to...
Need the answers to all of them. in its ground state? Which of the following atoms...
Need the answers
to all of them.
in its ground state? Which of the following atoms is paramagnetic B) bariwm (ba) O cadmium (Cd 1D) ymerbium (Yb) E) argon (Ar) 16. ー 17. Which of the following statenments is true? The kpion Is orbital is smaller than the helium is cebital because krypton's nuclear charge draws the electrons closer because krypton's p The krypton 1s oebital is smaller than the helium Is orbital and d orbitals crowd the s orbitals...
22. Select the correct statements below. L. An atom of chlorine is larger than sulfur because...
22. Select the correct statements below. L. An atom of chlorine is larger than sulfur because the addition of an electron increases the repulsions without an increase in attraction for the nucleus resulting in less screening. An atom of oxygen is smaller than an atom of carbon because the distance of the valence electrons remains the same while the attraction for the nucleus increases with increasing number of protons. III. An atom of potassium is smaller than an atom of...
answer a b or c Why is the atomic radius of magnesium ion much smaller than...
answer a b or c
Why is the atomic radius of magnesium ion much smaller than that of a neutral charged magnesium atom? (See the atomic radius graph) The magnesium ion's electrons require less space. No electrons are lost, they move to unoccupied spaces about the nucleus. The magnesium ion has fewer principle quantum energy levels, this causes a decrease in atomic radius. The magnesium ion has a higher Z-effective nuclear charge. The magnesium ion has more principle quantum energy...
1. Which element has larger Effective Nuclear Charge? Li or K I thought it would be...
1. Which element has larger Effective Nuclear Charge? Li or K I thought it would be Li because it has 2s1 as valence electron and this is closer to the nucleus with less shielding...would this not be the one with the highest effective nuclear charge. the answer says that its K which has a higher nuclear charge and this charge is countered by shielding of the core electrons but wouldn't K have a lower effective nuclear charge as it is...
Question 4 (1 point) Do you predict 52- or Ca2+ to have a smaller ionic radius? Why? Ca2+ is smaller because it has only two valence electrons whereas S2- has six. OCa2+ is smaller because its nucleus has a larger positive charge which exerts a stronger force than the nucleus of S2- on the same number of electrons. Os2- is smaller because it contains fewer electrons than Ca2+ and therefore has a smaller electron cloud. OS2- is smaller because it...
Question 10 4 pts Which of the following explanations best explains, from first principles, the fact that boron has a lower first ionization energy than beryllium? 0 Beryllium has more core electrons than boron. 0 Boron is more boring and hence it will be easier to remove the bored electrons from the shell. Electrons are more closely bound in beryllium because God invented the Octet Rule, such that beryllium is closer to an octet than boron. 0 In beryllium, an...
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...
Help with explanation if possible.
Nae Section -Date Now let's look at chlorine A chlorine atom has how many protons Therefore, we know that a chlorine atom has how many electrons? How many electrons will go in the first shell? How many in the second shell? Nucleus How many in the third? Draw this in Figure 2.2 We know that a chlorine atom requires eight electrons in its valence shell to become stable. Will it be easier for chlorine to...
Need the answers
to all of them.
in its ground state? Which of the following atoms is paramagnetic B) bariwm (ba) O cadmium (Cd 1D) ymerbium (Yb) E) argon (Ar) 16. ー 17. Which of the following statenments is true? The kpion Is orbital is smaller than the helium is cebital because krypton's nuclear charge draws the electrons closer because krypton's p The krypton 1s oebital is smaller than the helium Is orbital and d orbitals crowd the s orbitals...
22. Select the correct statements below. L. An atom of chlorine is larger than sulfur because the addition of an electron increases the repulsions without an increase in attraction for the nucleus resulting in less screening. An atom of oxygen is smaller than an atom of carbon because the distance of the valence electrons remains the same while the attraction for the nucleus increases with increasing number of protons. III. An atom of potassium is smaller than an atom of...
answer a b or c
Why is the atomic radius of magnesium ion much smaller than that of a neutral charged magnesium atom? (See the atomic radius graph) The magnesium ion's electrons require less space. No electrons are lost, they move to unoccupied spaces about the nucleus. The magnesium ion has fewer principle quantum energy levels, this causes a decrease in atomic radius. The magnesium ion has a higher Z-effective nuclear charge. The magnesium ion has more principle quantum energy...
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