ScienceChemistryChem M03
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Chem M03

Yaqub Clark avatar Yaqub Clark
25 July 2022
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84 test answers

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question
Group 8A elements have full outer principal s and p subshells.
answer
true
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The valence electrons of group 2A elements are in an s subshell.
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true
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Period 4 elements have an inner electron configuration of [Ar].
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true
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The highest principal energy level of period 2 elements is 2.
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true
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Period 5 elements have an inner electron configuration of [Xe].
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false
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Period 3 elements all have six 3p electrons.
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false
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The highest principal energy level of period 3 elements is 4.
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false
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The valence electrons of group 5A elements are in the 6s subshell.
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false
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Arrange the elements in decreasing order of the number of valence electrons.
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8: Ne, Ar 7: F, I, Cl 6: S 5: P, N 4: C 3: B 2: Ba, Be, Mg 1: Li, K
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Number the rows within each block of the periodic table according to the shell for the highest-energy electrons in an atom of those elements.
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1st column: 1s-7s 2nd column: 3d-6d 3rd column: 2p-7p bottom rows: 4f and 5f
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Use the orbital-filling diagram to show the electron configuration of phosphorus, PP.
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g2 : g1 3p: ^^^ 3s: i! 2p: i! i! i! 2s i! 1s i!
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Drag and drop orbitals and electron counts to complete the electron configuration of iron, FeFe.
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1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6
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1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
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Ba
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Which of the following groups comprise the s-block of elements?
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groups 1 and 2
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choose the 1s orbital
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blue circle; XYZ
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Choose the 2p orbital.
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pink ovals. two arms
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How would the 2s2s and 3p3p orbitals differ from the 1s1s and 2p2p orbitals?
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The 2s and 3p would have the same shape as the 1s and 2p. The only difference is that they would be larger in size.
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N
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1s^22s^22p^3
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Mg
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1s^22s^22p^63s^2
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Ar
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1s^22s^22p^63s^23p^6
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Se
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1s^22s^22p^63s^23p^64s^23d^104p^4
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Write the full orbital diagram for F.
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1s^2 2s^2 2p^5 1s i! 2s i! 2p i! i! i
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Indicate the number of unpaired electrons in F.
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1
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Write the full orbital diagram for C.
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1s^1 2s^2 2p^2 1s i! 2s i! 2p ii
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Indicate the number of unpaired electrons in C.
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2
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Write the full orbital diagram for Ne.
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1s^2 2s^2 2p^6 1s i! 2s i! 2p i! i! i!
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Write the full orbital diagram for Be
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1s^2 2s^2 2p 1s i! 2s i! 2p (nothing)
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Condense Te
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[Kr]5s^24d^105p^4
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Condense Br
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[Ar]4s^23d^104p^5
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Condense I
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[Kr]5s^24d^105p^5
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condence Cs
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[Xe]6s^1
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How many valence electrons are in Ba
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2
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How many valence electrons are in Al
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3
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How many valence electrons are in Be
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2
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How many valence electrons are in Se
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6
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How many valence electrons are in 3A
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ns^2np^1
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How many valence electrons are in 4A
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ns^2np^2
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How many valence electrons are in 6A
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ns^2np^4
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How many valence electrons are in 8A
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ns^2np^6
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Name an element in the third period (row) of the periodic table with 3 valence electrons.
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Aluminum
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Name an element in the third period (row) of the periodic table with a total of 4 3p electrons
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Sulfur
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Name an element in the third period (row) of the periodic table with 6 3p electrons.
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Argon
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Name an element in the third period (row) of the periodic table with 2 3s electrons and no 3p electrons.
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Magnesium
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[Ne]3s^1
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Sodium
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[Kr]5s^2 4d^10
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Cadmium
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[Xe]6s^2
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Barium
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[Kr]5s^2 4d^10 5p^3
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Antimony
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Select the correct electron-dot formulas
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N 1* F 7* Ne 8*
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Draw the electron-dot formula for the element sulfur.
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** ** S * *
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To form a stable ion, will magnesium gain or lose electrons? How many electrons?
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loose 2 electrons
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Match each ion with the noble gas whose electron configuration it shares.
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Helium Be^2+ Li+ Neon Na+ N^3- O^2- Argon Ca^2+ Cl- S^2-
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How many electrons are transferred between the cation and anion to form the ionic bond in one formula unit of each compound?
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1 Electron: KBr, LiF, NaCl 2 Electrons: BaS CaO
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Which of the following are valid ionic Lewis structures?
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Valid: Na+[Br]-, [F]- Ca^2+[F] Invalid: NaBr, [F]+Ca^2-[F]+ Na-[Br]+, FCaF
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Which nonmetals could form an ionic compound with magnesium with the formula MgX2MgX2 (where XX represents the nonmetal)?
answer
Possible: Br Cl F Not Possible: N O S
question
For neutral molecules, which statements about covalent Lewis structures are true?
answer
False: 1. Hydrogen atoms are often the central atom of a Lewis structure. 2. Each atom of a Lewis structure must have eight electrons. True 1. For a neutral molecule, the number of electrons in the Lewis structure is the sum of the valence electrons for the atoms. 2. Electrons of covalent compounds may be shared between atoms.
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A covalent compound is composed of a nitrogen atom, a hydrogen atom, and a carbon atom. How many electrons should the Lewis structure of the covalent compound contain?
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10
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What is the Lewis structure of the covalent compound that contains one nitrogen atom, one hydrogen atom, and one carbon atom?
answer
H-C ||| N **
question
Based on your answer above how many bonding electrons and lone pair electrons (nonbonding electrons) are there in the Lewis structure of HCNHCN?
answer
8,2
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Match each two-dimensional structure to its correct three-dimensional description.
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Linear: Y-X-Y Y=X=Y Trigonal Planar Y Y | | Y=X=Y Y-X-Y Bent ** ** Y-X-Y Y-X=Y ** Tetrahedral Y | Y-X-Y | Y Pyramidal Y | Y-X-Y **
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Classify these molecules as polar or nonpolar.
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polar: H2O, HF, CH3Br Non-polar: CBr4, CO2, N2
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Lewis dot diagram for Kr
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** ** K ** **
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Lewis dot diagram for P
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* *P* **
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Lewis dot diagram for B
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*B* *
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Lewis dot diagram for N
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N*
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Determine the electron geometry of N2O (oxygen is terminal).
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linear
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Determine the molecular geometry of N2O (oxygen is terminal).
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linear
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Determine the electron geometry of SO2
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trigonal planar
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Determine the molecular geometry of SO2
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bent
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Determine the electron geometry of H2S
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tetrahedral
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Determine the molecular geometry of H2S
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bent
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Determine the electron geometry of PF3
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tetrahedral
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Determine the molecular geometry of PF3
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trigonal pyramidal
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I2
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the molecule is nonpolar
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NO
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+ - N = O --------->
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HCl
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+ - H - Cl -------->
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N2
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nonpolar
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Find the electronegativity difference between K and Cl
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2.2
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Classify the bond that occurs between K and Cl
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ionic
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Classify the bond that occurs between N and N
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pure covalent
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Classify the bond that occurs between C and S
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Pure covalent
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Find the electronegativity difference between C and Cl
answer
0.5
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Classify the bond that occurs between C and Cl
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polar covalent
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Specify whether CH4 is polar, nonpolar, ionic, or polar covalent.
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nonpolar
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Draw the Lewis structure for CO
answer
C=-O