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Interpretation:
The electron configurations of magnesium and nickel are to be stated.
Concept introduction:
Electronic configuration represents the arrangement of electrons in an atom. The sublevels are filled according to their increasing energy. The electrons are firstly filled into the sublevel having the lowest energy. The sublevel closest to the nucleus has the lowest energy. The trend of filling of electrons according to the energy of sublevels is given below.
The electronic configuration up to the electronic configuration of the last noble gas is represented with the symbol of noble gas in square brackets. This notation is known as core notation.
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Chapter 11 Solutions
Introductory Chemistry: An Active Learning Approach
- How many sublevels are there in an atom with n=4?arrow_forwardAccording to the Bohr theory, which of the following would have the higher energy? a. An electron in an orbit close to the nucleus b. An electron in an orbit located farther from the nucleusarrow_forwardWithout looking at data in the text, sketch a qualitative graph of the third ionization energy versus atomic number for the elements Na through Ar, and explain your graph.arrow_forward
- Write complete electron configurations for atoms whose electron configurations end as follows. a. 3p5 b. 4d7 c. 4s2 d. 3d1arrow_forwardDraw electron configurations for each of the following elements according to the Bohr model. Indicate which electrons are valence electrons. a. Mg b. S c. He d. Karrow_forwardWrite complete electron configurations for atoms whose electron configurations end as follows. a. 4p2 b. 3d10 c. 5s1 d. 4p6arrow_forward
- Indicate whether each of the following statements is true or false. If false, correct the statement. (a) An electron transition from n=3 to n=1 gives off energy. (b) Light emitted by an n=4 to n=2 transition will have a longer wavelength than that from an n=5 to n=2 transition. (c) A sublevel of l=3 has a capacity of ten electrons. (d) An atom of Group 13 has three unpaired electrons.arrow_forwardThe four most abundant elements by mass in the human body are oxygen, carbon, hydrogen, and nitrogen. These four elements make up about 96% of the human body. The next four most abundant elements are calcium, phosphorus, magnesium, and potassium. Excluding hydrogen, which of these elements would have the smallest size? largest size? smallest first ionization energy? largest first ionization energy?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_forward
- 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_forwardWrite the full electron configuration (1s32s2,etc.) for each of the following elements. phosphorus, Z=15 calcium, Z=20 potassium, Z=19 boron, Z=5arrow_forwardWrite the complete orbital diagram for each of the following elements, using boxes to represent orbitals and arrows to represent electrons. helium, Z=2 c. krypton, Z=36 neon, Z=10 d. xenon, Z=54arrow_forward
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