(a)
Interpretation:
The given statement about valence electrons of atoms of main-group elements is a true statement or not is to be identified and if the statement is false, it is to be changed into a true statement.
(b)
Interpretation:
The given statement about valence electrons of atoms of main-group elements is a true statement or not is to be identified and if the statement is false, it is to be changed into a true statement.
(c)
Interpretation:
The given statement about valence electrons of atoms of main-group elements is a true statement or not is to be identified and if the statement is false, it is to be changed into a true statement.
(d)
Interpretation:
The given statement about valence electrons of atoms of main-group elements is a true statement or not is to be identified and if the statement is false, it is to be changed into a true statement.
(e)
Interpretation:
The given statement about valence electrons of atoms of main-group elements is a true statement or not is to be identified and if the statement is false, it is to be changed into a true statement.
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INTRODUCTION TO CHEMISTRY-CONNECT ACCESS
- Determine whether each statement that follows is true or false: a Electron energies are quantized in excited states but not in the ground state. b Line spectra of the elements are experimental evidence of the quantization of electron energies. c Energy is released as an electron passes from ground state to an excited state. d The energy of an electron may be between two quantized energy levels. e The Bohr model explanation of line spectra is still thought to be correct. f The quantum mechanical model of the atom describes orbitals in which electrons travel around the nucleus. g Orbitals are regions in which there is a high probability of finding an electron. h All energy sublevels have the same number of orbitals. i The 3p orbitals of an atom are larger than its 2p orbitals but smaller than its 4p orbitals. j At a given sublevel, the maximum number of d electrons is 5. k The halogens are found in Group 7A/17 of the periodic table. l The dot structure of the alkaline earths is X, where X is the symbol of element in the family. m Stable ions formed by alkaline earth metals are isoelectronic with noble gas atoms. n Atomic numbers 23 and 45 both belong to transition elements. o Atomic number 52, 35, and 18 are arranged in order of increasing atomic size. p Atomic number 7, 16, and 35 are all nonmetals.arrow_forwardHow are the Bohr model and the Rutherford model of the atom similar? How are they different?arrow_forwardWhich orbital is the first be filled in any atom? Why?arrow_forward
- Explain electron from a quantum mechanical perspective, including a discussion of atomic radii, probabilities, and orbitals.arrow_forwardr Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.arrow_forwardWhich atom would be expected to have a half-filled 4s subshell?arrow_forward
- Write the valence-electron configuration of each of the following elements, basing your answer on the element’s location on the periodic table. uranium, Z=92 c. mercury, Z=80 manganese, Z=25 d. francium, Z=87arrow_forwardHow are the Bohr model and the quantum mechanical model of the hydrogen atom similar? How are they different?arrow_forward
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