Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer nur like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions t complete the table. electron configuration of atoms location of elements (check all that apply) blocks metals or nonmetals? Os Op [G]ns² mdo np 10 3 Od Of [G]² np metals O nonmetals metalloids O metals 6 Os Op O nonmetals Od Of O metalloids [G]ns Os Op Od Of metals O nonmetals 000 metalloids

Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer nur like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions t complete the table. electron configuration of atoms location of elements (check all that apply) blocks metals or nonmetals? Os Op [G]ns² mdo np 10 3 Od Of [G]² np metals O nonmetals metalloids O metals 6 Os Op O nonmetals Od Of O metalloids [G]ns Os Op Od Of metals O nonmetals 000 metalloids

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. y For an electron in the 2s orbital shown above, enter a possible value for each quantum number. n = 1 = Give ONE example. Give ONE example. Though a given electron only has one value for possible mi, there are my values for electrons in 2s orbitals. m = m = Submit Answer Retry Entire Group 9 more group attempts remaining
An unidentified element is known to have an electron configuration, [X] ns^2, in its ground state. This element must be in the same family as… A) arsenic B) lead C) radon (Rn) D) rubisium (rb) E) radium (Ra)
Write the electron configurations for the following atoms. Do not use shorthand notation, and use parenthesis. Do not put spaces in your answer. For example, enter the configuration for Na as 1s(2)2s(2)2p(6)3s(1). As: Cl: Ni: Si: NOV
The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. For an electron in the 3p orbital shown above, enter a possible value for each quantum number. n = 1 = = Give ONE example. Give ONE example. Though a given electron only has one value for possible mi, there are my values for electrons in 3p orbitals. m₁ = mg = Submit Answer Retry Entire Group 9 more group attempts remaining
Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions to complete the table. electron configuration of atoms 6 [G]ns²np [G]ns¹ 2 [G]ns²mf³ 3 blocks 00 P S 00 P 00 S location of elements (check all that apply) S C р р f р f metals or nonmetals? 000 000 000 metals nonmetals metalloids metals nonmetals metalloids metals nonmetals metalloids
Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions to complete the table. electron configuration of atoms 2 [G]ns²mfs 5 3 [G]ns² md¹np³ [G]ns²md¹np 6 blocks 00 00 S e S S location of elements (check all that apply) a U 0 00 р f р f р f metals or nonmetals? 00 000 0 0 0 X metals nonmetals metalloids metals nonmetals metalloids metals nonmetals metalloids Ś
3. A student was asked to write the electron configuration for a number of elements on an exam. Here is a sample of some of their answers: a) Ne s2 b) 1s²25³ c) [Kr] 4s1 Select any 2 of the answers above, and explain what is wrong. What element do you think they were describing? Write the correct electron configuration for that element.
In a given atom, what are the maximum number of electrons that are allowed to have the following sets of quantum number? If you could explain at least 2-3 to me (no matter the order, I would really appreciate it.
Give typed full explanation not a single word hand written otherwise leave it
Write full electron configurations for Ge. Express your answer in complete form in the order of orbital filling as a string without blank space between orbitals. For example, 1s22s21s22s2 should be entered as 1s^22s^2. Write full electron configurations for Cl. Express your answer in complete form in the order of orbital filling as a string without blank space between orbitals. For example, 1s22s21s22s2 should be entered as 1s^22s^2. Write full electron configurations for Sr. Express your answer in complete form in the order of orbital filling as a string without blank space between orbitals. For example, 1s22s21s22s2 should be entered as 1s^22s^2.
The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. In progress For an electron in the 3s orbital shown above, enter a possible value for each quantum number. n = 1 = = Give ONE example. Give ONE example. Though a given electron only has one value for possible mi, there are my values for electrons in 3s orbitals. m₁ = ms = Submit Answer Retry Entire Group 9 more group attempts remaining