Chemistry

Chemistry, 24.09.2019 11:30, kalebrayburn62

In ammonia, a central nitrogen atom is bonded to three hydrogen atoms. similarly, boron trifluoride has a central boron atom bonded to three fluorine atoms. however, ammonia is pyramidal and boron trifluoride is trigonal planar in shape. which statement justifies this difference in their structure?

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Chemistry, 27.07.2019 17:30, nockturnal1993

In ammonia, a central nitrogen atom is bonded to three hydrogen atoms. similarly, boron trifluoride has a central boron atom bonded to three fluorine atoms. however, ammonia is pyramidal and boron trifluoride is trigonal planar in shape. which statement justifies this difference in their structure? the lone pair of electrons in boron trifluoride increases the bond angle between the bonding pairs, giving it a planar structure. the lone pair of electrons in boron trifluoride decreases the bond angle between the bonding pairs, giving it a planar structure. the lone pair of electrons in boron trifluoride stabilizes the bond angle between the bonding pairs, giving it a planar structure. the lone pair of electrons in ammonia increases the bond angle between the bonding pairs, giving it a pyramidal structure. the lone pair of electrons on the nitrogen in ammonia decreases the bond angle between the bonding pairs, giving it a pyramidal structure.

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Physics, 24.08.2019 21:00, nosugh

In ammonia, a central nitrogen atom is bonded to three hydrogen atoms. similarly, boron trifluoride has a central boron atom bonded to three fluorine atoms. however, ammonia is pyramidal and boron trifluoride is trigonal planar in shape. which statement justifies this difference in their structure? a. the lone pair of electrons in boron trifluoride increases the bond angle between the bonding pairs, giving it a planar structure. b. the lone pair of electrons in boron trifluoride decreases the bond angle between the bonding pairs, giving it a planar structure. c. the lone pair of electrons in boron trifluoride stabilizes the bond angle between the bonding pairs, giving it a planar structure. d. the lone pair of electrons in ammonia increases the bond angle between the bonding pairs, giving it a pyramidal structure. e. the lone pair of electrons on the nitrogen in ammonia decreases the bond angle between the bonding pairs, giving it a pyramidal structure.

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Chemistry, 08.10.2019 20:00, marykayy0218own5cp

1.) what is the steric number and the bond angles associated with each of the following molecules if a is the central atom, x refers to the atoms bonded to it and there are no lone pairs on the central atom. ax3 ax4 ax6 2.)what is the electron domain geometry of the following molecules? brcl5 bcl3 ph3 3.)which of the following molecules has a trigonal planar structure? co32− socl2 h3o+ so32 4.)the following geometries are possible for a molecule with three atoms bonded to a central atom assuming the bonded atoms are halogens, determine the central atom for each of these molecular geometries choosing from one of the following atoms. be, al, br, or as, 5.)put the following three molecules in order of increasing h—x—h bond angle, where x is the central atom. ch4 h2s ph3 ch4 < h2s < ph3 h2s < ph3 < ch4 ch4 < ph3 < h2s h2s < ch4 < ph3 ph3 < ch4 < h2s if you can can you also provide explanation you

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In ammonia, a central nitrogen atom is bonded to three hydrogen atoms. similarly, boron trifluoride...

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