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- Draw Lewis diagrams for the following compounds. In the formula the symbol of the central atom is given first. (Hint: The valence octet may be expanded for the central atom.) (a) PF5 (b) SF4 (c) XeO2F2help on all 3 parts of this question please. every time o go to submitt it its saying I put them in the wrong order. A) Arrange the following elements in order of increasing electronegativity:iodine, bromine, astatine, chlorine B) Arrange the following elements in order of increasing electronegativity:carbon, germanium, silicon, tin C)Arrange the following elements in order of increasing electronegativity:cesium, lead, thallium, bariumFind ways to demonstrate the 12 VSEPR SHAPES , non bonding electrons must be included! Use given chart and fill thanks
- Write a brief explanation of the graph for Electronegativity you saw in the activity. Be specific about the trend of electronegativity and how it relates to areas of the periodic table. I’ll put the image belowcan you explain a little bit about the rules when drawing lewis dot diagrams, it is correct to say that all elements need 8 electrons to be stable and if their is extrea valance electrons this gets added to the center atom and if not eneough creat double bonds.For each of the given below, compute for the electronegativity difference (2 decimal places) and identify the bond type of the compound write PC for polar covalent, and NPC for nonpolar covalent, and IB for ionic bond. Refer to the sample shown below
- These are topics for my quiz, I need one example from each. identify compounds as molecular or ionic from formula and electronegativity trends on period table compare, contrast physical properties of ionic vs. molecular compounds write formulas for "complicated" ionic compoundsUse the figure to find the electronegativity difference between each of the following pairs of elements, then use the table below to classify the bonds that occur between them as pure covalent, polar covalent, or ionic. (Electronegativity of CrCr is 1.6) Electronegativity Difference (ΔENΔEN) Bond Type Example zero (0−0.40−0.4) pure covalent Cl2Cl2 intermediate (0.4−2.00.4−2.0) polar covalent HFHF large (2.0+2.0+) ionic NaClNaCl Find the electronegativity difference between Si and O. Express your answer using two significant figures.Use the figure to find the electronegativity difference between each of the following pairs of elements, then use the table below to classify the bonds that occur between them as pure covalent, polar covalent, or ionic. (Electronegativity of CrCr is 1.6) Electronegativity Difference (ΔENΔEN) Bond Type Example zero (0−0.40−0.4) pure covalent Cl2Cl2 intermediate (0.4−2.00.4−2.0) polar covalent HFHF large (2.0+2.0+) ionic NaClNaCl Find the electronegativity difference between Br and Br. Express your answer using two significant figures.
- Use the figure to find the electronegativity difference between each of the following pairs of elements, then use the table below to classify the bonds that occur between them as pure covalent, polar covalent, or ionic. (Electronegativity of CrCr is 1.6) Electronegativity Difference (ΔENΔEN) Bond Type Example zero (0−0.40−0.4) pure covalent Cl2Cl2 intermediate (0.4−2.00.4−2.0) polar covalent HFHF large (2.0+2.0+) ionic NaClNaCl Find the electronegativity difference between Mg and Br. Express your answer using two significant figures.Give me a clear handwritten answer with explanation...please give answer all sub parts...give short explanation associate the molecules and ions below with yheir correct molecular shape such as linear, trigonal pyrimidal, trigonal planar, bent, or tetrahedralCould someone help me?? The answer to this question must look similar to the example attached. Back ground info: Atoms of different elements combine with one another to form compounds. It is important to be able to explain how atoms actually come together to form these compounds or chemical bonds. One of the three types of bonds is an ionic bond which is a bond between a metal atom and a nonmetal atom, or a cation and an anion. The Octet Rule is the driving force behind ionic bond formation. The octet rule refers to the tendency of atoms to prefer to have eight electrons in the valence shell. When atoms have fewer than eight electrons, they tend to react and form more stable compounds. When discussing the octet rule, we do not consider d or f electrons. Only the s and p electrons are involved in the octet rule, making it useful for the main group elements (elements not in the transition metal or inner-transition metal blocks); an octet in these atoms corresponds to an electron…