To determine: The number of electrons in a fluorine atom.
Concept introduction: The atomic number of an element is the number of protons in the nucleus of its atoms. In a neutral atom, the number of protons and electrons is equal. Thus, the number of electrons present in a neutral atom is equal to its atomic number.
To determine: The number of shells in a fluorine atom.
Concept introduction: The electrons in an atom present around the nucleus are in constant motion. An electronic shell represents the energy levels and the average distance at which electrons orbit around the nucleus. Simplified diagrams of atoms show the electrons arranged in electronic shells as concentric rings around the nucleus. In an atom, the first shell can contain only two electrons, whereas the second shell can have a total of 8 electrons.
To list: The names of orbitals occupied by electrons in a fluorine atom.
Concept introduction: Electronic shells can be subdivided into electronic orbitals. Each electronic orbital represents the three-dimensional volume around the nucleus where an electron is most likely to occur while orbiting around the nucleus. Each orbital can have two electrons. Thus, the number of electrons present in each shell depends on the number of orbitals in each shell. In an atom, the first shell has one orbital called 1s, thus it can contain only two electrons. The second shell has one spherical orbital called 2s, and three dumbbell shaped orbitals named 2p orbitals (Fig. 2). Thus, the second shell can have a total of 8 electrons.
To determine: The number of electrons needed to completely fill the valence shell of a fluorine atom.
Concept introduction: The outermost shell of an atom is called the valence shell, and the electrons present in it are called valence electrons.
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
EBK CAMPBELL BIOLOGY
- What is the net charge on the following tripeptides (single-letter abbreviations). * YLV at pH 10.9 (the answer is -1.5 but I don't understand why)arrow_forwardif the 3 to 1 transition has an energy of 1.94x10^-18 J what do you think the energy of the 1 to 3 transition is explain whyarrow_forward1) Explain how g orbitals are different from s, p, d, and f atomic orbitals? - determine the number of g orbitals that will exist in a given energy level? - include a set of quantum numbers (n, l, and ml) for one of the g orbitals in the lowest energy set of g orbitals? 2) TlF3 forms a stable compound, while the similar compounds TlCl3 and TlBr3 are unstable and undergo disproportionation. Explain why the fluoro compound is more stable than the chloro and boromo compounds?arrow_forward
- write the orbital box diagram and dipole moment using the lewis strcuture for clo3^-: orbital name, bonds and lone pairsarrow_forwardpKa = 9.6 pK, = 2.3 H :0: || H-N- C-C-Ö-H H 120° 180° H H 20. 105° The structural formula of the glycinium cation is shown above. Arrows indicate the pka values for the labile 90° protons in the molecule. CLEAR ALL What is the approximate H-O-C bond angle in the glycinium cation? +arrow_forwardI Review | Constants | Periodic Table You may want to reference (Page) Section 9.5 while completing this problem. Propane (C3 H8) burns in oxygen to produce carbon dioxide and water via the following reaction: C3HS (g) + 502 (g)→3CO2 (g) + 4H,0(g) Part A Calculate the mass of CO2 that can be produced if the reaction of 37.3 g of propane and sufficient oxygen has a 56.0 % yield. Express your answer with the appropriate units. l'i HẢ ? m(CO,) = Value Units Submit Request Answer Provide Feedback Next >arrow_forward
- H₂C-C Ö: CH2 H3C — с O CH₂ + Clear The Lewis structure of acetone enolate ion, which has one other resonance structure, is shown. Complete the resonance structure by dragging bonds, charges, and electron lone pairs to their appropriate positions. Then check your answer.arrow_forwardA compound with empirical formula C2H5O was found in a separate experiment to have a molar mass of approximately 90 g. What is the molecular formula of the compound?arrow_forwardLook up the valence electron configuration, covalent atomic radius, effective nuclear charge, first ionization energy and Pauling electronegativity in Chapter 8 (tables are attached). Examine the above data and answer the following questions. a) Explain why some of the elements like TI and Pb on the lower left of the p block are metallic. b) Explain why some of the elements like C, Si in the center of the p block form covalent bonds. Explain why these bonds formed by the network of these elements (as studied in Chapter 25) tend to be unreactive. c) Explain why the noble Group 8A elements are highly unreactive gases. d) Explain why some elements like F, CI, Br etc, on the upper right of the p block are highly reactive nonmetals.arrow_forward
- Butadiene (right) is a colorless gas used to make synthetic rubber and many other compounds. (a) How many σ bonds and π bonds does the molecule have? (b) Are cis-trans arrangements about the double bonds possible? Explain.arrow_forwardHow many electrons are in the outer shell of each of the following atoms?arrow_forwardConstants I Periodic Table Given the data in the table below, calculate the bond enthalpy and energy at 298.15 K of the following: Completed Substance Formula Part B (kJ · mol-1) Carbon (g) 716.7 The C-C single bond in C3 H6 (cyclopropane) (use C-H bond enthalpy and bond energy calculated for CH4). Hydrogen (g) H 218.0 Methane (g) CH4 -74.6 Express your answers in kilojoules per mole to three significant figures separated by a comma. Ethane (g) C2H6 -84.0 Propane (g) C3 Hs ν ΑΣφ -103.8 Cyclopropane (g) C3 H6 53.3 Ethene (g) C2H4 52.4 Bond enthalpy, bond energy = kJ . mol-1 Ethyne (g) C2H2 227.4 Submit Request Answerarrow_forward
- Principles Of Radiographic Imaging: An Art And A ...Health & NutritionISBN:9781337711067Author:Richard R. Carlton, Arlene M. Adler, Vesna BalacPublisher:Cengage Learning