Concept explainers
(a)
Interpretation:
The ground state electronic configuration for
Concept Introduction:
- Excited state electronic configuration:
The electronic configuration that results when an electron in the ground state have been moved to a higher –energy orbital.
- Ground state electronic configuration:
A description about orbitals in which the electrons of an atom occupies when they are all in their lowest available energy orbital.
Electron configuration: The distribution of electrons of an atom or molecule in atomic or molecular orbitals.
Formation of ions:
Atom possesses equal number of protons and electrons and remains electrically neutral. By gaining (accepting electrons) or losing (donating electrons) one or more electrons, converts the neutral atom into a charged particle called IONS.
Cation: The loss of one or more electrons by a neutral atom leaves the atom positively charged called cation.
Anion: The gain of one or more electrons by a neutral atom leaves the neutral atom negatively charged called anion.
(b)
Interpretation:
The ground state electronic configuration for
Concept Introduction:
- Excited state electronic configuration:
The electronic configuration that results when an electron in the ground state have been moved to a higher –energy orbital.
- Ground state electronic configuration:
A description about orbitals in which the electrons of an atom occupies when they are all in their lowest available energy orbital.
Electron configuration: The distribution of electrons of an atom or molecule in atomic or molecular orbitals.
Formation of ions:
Atom possesses equal number of protons and electrons and remains electrically neutral. By gaining (accepting electrons) or losing (donating electrons) one or more electrons, converts the neutral atom into a charged particle called IONS.
Cation: The loss of one or more electrons by a neutral atom leaves the atom positively charged called cation.
Anion: The gain of one or more electrons by a neutral atom leaves the neutral atom negatively charged called anion.
(c)
Interpretation:
The ground state electronic configuration for
Concept Introduction:
- Excited state electronic configuration:
The electronic configuration that results when an electron in the ground state have been moved to a higher –energy orbital.
- Ground state electronic configuration:
A description about orbitals in which the electrons of an atom occupies when they are all in their lowest available energy orbital.
Electron configuration: The distribution of electrons of an atom or molecule in atomic or molecular orbitals.
Formation of ions:
Atom possesses equal number of protons and electrons and remains electrically neutral. By gaining (accepting electrons) or losing (donating electrons) one or more electrons, converts the neutral atom into a charged particle called IONS.
Cation: The loss of one or more electrons by a neutral atom leaves the atom positively charged called cation.
Anion: The gain of one or more electrons by a neutral atom leaves the neutral atom negatively charged called anion.
(d)
Interpretation:
- Excited state electronic configuration:
The electronic configuration that results when an electron in the ground state have been moved to a higher –energy orbital.
- Ground state electronic configuration:
A description about orbitals in which the electrons of an atom occupies when they are all in their lowest available energy orbital.
Electron configuration: The distribution of electrons of an atom or molecule in atomic or molecular orbitals.
Formation of ions:
Atom possesses equal number of protons and electrons and remains electrically neutral. By gaining (accepting electrons) or losing (donating electrons) one or more electrons, converts the neutral atom into a charged particle called IONS.
Cation: The loss of one or more electrons by a neutral atom leaves the atom positively charged called cation.
Anion: The gain of one or more electrons by a neutral atom leaves the neutral atom negatively charged called anion.
Want to see the full answer?
Check out a sample textbook solutionChapter 1 Solutions
Essential Organic Chemistry (3rd Edition)
- The electronic structure 1s2s22p63s23p64s23d104p65s24d6 refers to the ground state of Xe Ru. Rh. O Tc. O Fe.arrow_forwardConfigurations that is NOT paramagnetic a. 1s2 2s2 2p6 3s2 3p5 b. 1s2 2s2 2p6 3s2 3p6 c. 1s2 2s2 2p6 3s2 3p4 d. 1s2 2s2 2p6 3s7arrow_forwardThe sun is a giant nuclear reactor, which emits light (electromagnetic radiation) at a range of frequencies. We human can only see visible light (400 – 700 nm), because its absorption results in a conformational change in the retinal molecule, which triggers a neural signal. a. What is the frequency of a 500 nm visible photon? b. How much energy in J does a 500 nm visible photon carry? A typical chemical bond has an energy of 5x10-19 J. Would a visible photon at 500 nm be С. sufficient to break a chemical bond? d. How about a UV (200 nm) photon? Indeed, UV light can damage DNA, the genetic material in our body, leading to mutations and possibly cancer.arrow_forward
- Br Br Br H. Br H. Structure B Structure C Structure D Structure E Structures B and C are: Choose... Structures B and D are: Choose... Structures B and E are: Choose... Structures C and E are: Choose... Structures C and D are: Choose... Structures D and E are: Choose... ...Oarrow_forwardAHCN + 50 2(g) 2H2OG) + 4CO2(9) + 2N2 Calculate AS using the table provided. Compound S re HCN HČN 94.1 205.0 H,0 189.0 214 192arrow_forward93. Which of the following is mismatched? a. Mg - p block b. S- p block c. Na - s block d. Fe - d blockarrow_forward
- Question 7 Which of the following statements describe phosphorescence? O A. takes place when when electron in excited energy is released and the molecules comes back in ground state from singlet excited state B. Emmission of light by a subsatnce that has absorbed light O C.high energy release O D. the emission of a photon during a transition between states with metasable state/ tripletarrow_forwardE Miracle Hudson - DR- Bonding G Why do elements of Groups 1 a cs.google.com document/d/10ufqxTulDjB3XC3b8VW9M94mNac0TaEeTOJjHY9rjxE/edit ular Ty. H The Amazonian Ex. How Theodore Roo DAREBEE Workouts Skyward G Login - Powered by. 7- DR- Bonding Chapter 1:2 Insert Format Tools Add-ons Help Last edit was seconds ago 0% Normal text Comlc San. в I U A > 12 E E = E + 1 3 Ionic Bonds (p. 8-11) 1) An atom that loses one or more electrons from its outermost energy level becomes a positivel charged ion. 2) Which of the following elements give up electrons to other atoms? (Highlight ALL that apply) True or False? a) Sodium b) Aluminum c) Chlorine d) Oxygen 3) Why do elements of Groups 1 and 2 react so easily? 4) The names of negative ions that form when atoms gain electrons have the ending 5) Which of the following are common properties of an ionic compound? (Highlight ALL that apply) a) Its solid form is a crystal lattice b) It contains alternating positive and negative ions c) It is soft and…arrow_forwardHNO, H2SO, NO2 A. correct regioselectivity B. incorrect regioselectivity a. choice A. Ob.choice B.arrow_forward
- Draw the molecular orbital diagram of the following: Given options are : a. C22- b. H22- c. Ne2+ d. O22+ Please write it in nice handwriting thank youarrow_forwardDoes the minimization of electron-electron repulsions correlate with Hund's rule?arrow_forward43. H2S Match the family of elements with the properties listed. (p16) 44. Highest ionization energy a. metals b. non-metals c. inert gases 45. Valence electrons are easily removed a. metals b. non-metals c. inert gases 46. Electron cloud is full, rarely reacts a. metals b. non-metals c. inert gases 47. Good conductor of heat and electricity a. metals b. non-metals c. inert gases 48. Malleable a. metals b. non-metals c. inert gases Is the predominant type of bonding ionic, covalent, or metallic? (p13-14) 49. NaCl a. ionic b. covalent C. metallic 50. H20 a. ionic b. covalent c. metallicarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning