Why aren't heavier elements much larger than lighter elements? Why aren't heavier elements much larger than...
Why aren't heavier elements much larger than lighter elements?
Why aren't heavier elements much larger than lighter elements?
| Larger nuclear forces pull the electrons into closer orbits. |
| Larger gravitational forces pull electrons into closer orbits. |
| The larger positive charge in the nucleus pulls the electrons into closer orbits. |
| Larger magnetic forces pull electrons into closer orbits. |
Homework Answers
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Why aren't heavier elements much larger than lighter
elements?
Why aren't heavier elements much larger than...
Why is the effective nuclear charge seen by valence electrons much less than Zq? A. Filled...
Why is the effective nuclear charge seen by valence electrons much less than Zq? A. Filled shells below valence electrons neutralize some of the proton charge. B. The valence electrons are further away from the nucleus. C. There are fewer valence electrons than nuclear protons. D. The valence electrons have less charge themselves.
D Question 10 Why is Bra smaller atom than As? Br is actually larger than As...
D Question 10 Why is Bra smaller atom than As? Br is actually larger than As because it has more protons. As is larger because it has more protons and electrons. Br has more protons to pull the electrons in closer. Br is smaller because it has less protons and electrons making it smaller. Br is actually larger than As because it has a larger atomic mass. Question 11 Explain why metals have lower ionization energy than nonmetals. No answer...
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...
Each of the statements below attempts to explain why some periodic property varies predictably among elements...
Each of the statements below attempts to explain why some periodic property varies predictably among elements in the periodic table. Determine if each statement is true or false. True False Within a family, elements with higher atomic numbers have atoms of larger radius because the atoms have lower effective nuclear charge. True False Within a period, elements with lower atomic numbers have lower electronegativity because the valance electrons are in higher principal energy levels. True False Within a family, elements with lower atomic...
The boiling point of iodine (12) is much higher than the boiling point of helium (He)....
The boiling point of iodine (12) is much higher than the boiling point of helium (He). Why? O 12 has a larger electron cloud than He, so more energy is required to overcome the stronger London Dispersion Forces. O It requires more energy to break the covalent bonds in 12 than to overcome the London Dispersion Forces between He atoms. The bonds between iodine atoms are stronger than the bonds between helium atoms and therefore harder to break. O 12...
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...
Why do you think that the enthalpy of vaporization for water is so much larger than...
Why do you think that the enthalpy of vaporization for water is so much larger than the enthalpy of fusion? Hint: Think about intermolecular forces.
(b) Why is the magnitude of this value so much larger than the heat of vaporization...
(b) Why is the magnitude of this value so much larger than the heat of vaporization of water (AH°vap = 41 kJ/mol)? * Choose one: A. Less energy is needed to form attractive forces between water molecules than to break H-H and O-O bonds and form H-O bonds. O B. More energy is needed to form attractive forces between water molecules than to break H-Hand O-O bonds and form H-O bonds. o C. Less energy is needed to break attractive...
Why are there more retro-elements that generally account for a larger fraction of the genome than...
Why are there more retro-elements that generally account for a larger fraction of the genome than there are transposable elements like the Ac/Ds elements of maize, a simple DNA transposon?
Why are there more retro-elements that generally account for a larger fraction of the genome than...
Why are there more retro-elements that generally account for a larger fraction of the genome than there are transposable elements like the Ac/Ds elements of maize, a simple DNA transposon?
D Question 10 Why is Bra smaller atom than As? Br is actually larger than As because it has more protons. As is larger because it has more protons and electrons. Br has more protons to pull the electrons in closer. Br is smaller because it has less protons and electrons making it smaller. Br is actually larger than As because it has a larger atomic mass. Question 11 Explain why metals have lower ionization energy than nonmetals. No answer...
The boiling point of iodine (12) is much higher than the boiling point of helium (He). Why? O 12 has a larger electron cloud than He, so more energy is required to overcome the stronger London Dispersion Forces. O It requires more energy to break the covalent bonds in 12 than to overcome the London Dispersion Forces between He atoms. The bonds between iodine atoms are stronger than the bonds between helium atoms and therefore harder to break. O 12...
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...
(b) Why is the magnitude of this value so much larger than the heat of vaporization of water (AH°vap = 41 kJ/mol)? * Choose one: A. Less energy is needed to form attractive forces between water molecules than to break H-H and O-O bonds and form H-O bonds. O B. More energy is needed to form attractive forces between water molecules than to break H-Hand O-O bonds and form H-O bonds. o C. Less energy is needed to break attractive...
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