



Study with the several resources on Docsity
Earn points by helping other students or get them with a premium plan
Prepare for your exams
Study with the several resources on Docsity
Earn points to download
Earn points by helping other students or get them with a premium plan
Community
Ask the community for help and clear up your study doubts
Discover the best universities in your country according to Docsity users
Free resources
Download our free guides on studying techniques, anxiety management strategies, and thesis advice from Docsity tutors
Lewis dot structure Krypton Lewis structure Phosphorus valence electrons Boron electron configuration Sodium Lewis dot structure valence electrons in krypton electron configuration for phosphorus silver Lewis dot structure covalent bonding nonmetals
Typology: Exams
1 / 5
This page cannot be seen from the preview
Don't miss anything!
Draw the Lewis dot structure for Kr. To change the symbol of an atom, dou- ble-click on the atom and enter the letter of the new atom.: 8 E Kr Correct In the Lewis model, the valence electrons of main-group elements are represented as dots surrounding the symbol of the element. Each dot represents a valence electron. You place the dots around an element's symbol with a maximum of two dots per side. Kr has the electron configuration n [Ar]4s2 4p6. Therefore, Kr has eight valence electrons.
Draw the Lewis dot structure for P.: 5 E FOR P Spread them around the atom and then double up. Correct P has the electron configuration [Ne] 3s2 3p3. Therefore, P has five valence electrons.
Draw the Lewis dot structure for B. To change the symbol of an atom, dou- ble-click on the atom and enter the letter of the new atom.: Correct B has the electron configuration [He] 2s2 2p1. Therefore, B has three valence electrons.
Draw the Lewis dot structure for Na. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom.: 1 e for na Correct NaNa has the electron configuration [Ne]3s1[Ne]3ý1. Therefore, NaNa has one valence electron.
Se Express your answer as a chemical symbol.: Kr
I: Xe
Sr2+: Kr because Sr2+ indicates an Sr ion that has lost 2 E making it have the same # of Es as Kr
F: Ne
combine to create a compound, the transfer of electrons generates an ionic bond.:
Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.: The sharing of electrons between ele- ments generates the compound CH4, thus forming covalent bonds. Four hydrogen atoms each share one electron with carbon to create stable outer shells for all atoms.
NF3: The sharing of electrons between elements generates the compound NF3NF3, thus forming covalent bonds. One nitrogen atom shares one electron with each of the three fluorine atoms to form stable outer shells for all atoms.
OF3: Correct The sharing of electrons between elements generates the compound OF2OF2, thus forming covalent bonds. One oxygen atom shares one electron with each of the two fluorine atoms to form stable outer shells for all atoms.
Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.: The sharing of electrons between elements generates the compound H2OH2O, thus forming covalent bonds. One
= 16 tot Distribute electrons among the atoms, giving octets to as many atoms as possible. If any atoms lack an octet, as they do in this case, form double bonds as necessary to give them octets. Recall that electron groups are lone pairs, single bonds, or multiple bonds. SiO2 has the following structure: The central atom has two bonding groups and no lone pairs. Therefore, the molecular geometry is linear.:
BF3 contains 24 electrons: total number of electrons for Lewis structure = (#valenceeforB) + (#valencee - forF) = 3 + 3(7) = 24 Distribute electrons among the atoms, giving octets to as many atoms as possible. A significant exception to the octet rule is boron, which tends to form compounds with only six electrons around the central BB atom. Recall that electron groups are lone pairs, single bonds, or multiple bonds. BF3 has the following structure: The central atom has three bonding groups and no lone pairs. Therefore, the molecular geometry is trigonal planar.:
atom.): tetrahedral
CFCl3 contains 24 electrons: totalnumberofelectronsforLewisstructure = (#valenceeforC)+(#valencee - forF)+(#valenceeforCl) = 4+7+3(7) = 32 Distribute electrons among the atoms, giving octets to as many atoms as possible. Recall that electron groups are lone pairs, single bonds, or multiple bonds. CFCl3 has the following structure:
The central atom has four bonding groups and no lone pairs. Therefore, the molecular geometry is tetrahedral.:
central atom): trigonal planar
H2CS contains 12 electrons: totalnumberofelectronsforLewisstructure = (#valenceeforH)+(#valencee - forC)+(#valenceeforS) = 2(1) + 4 + 6 = 12 Distribute electrons among the atoms, giving octets (or duets for hydrogen) to as many atoms as possible. If any atoms lack an octet, as in this case, form double or triple bonds as necessary to give them octets. Recall that electron groups are lone pairs, single bonds, or multiple bonds. H2CSH2CS has the following structure: The central atom has three bonding groups and no lone pairs. Therefore, the molecular geometry is trigonal planar.: