chemical bonding and molecular geometry

PPTX 64 pages 3.7 MB Free download

64 pages

FaylHub.uz

Download via Telegram

Size 3.7 MB

File type PPTX

Pages 64

Updated Dec 2025

Page preview (5 pages)

Scroll down 👇

1 / 64

8.1 types of chemical bonds 6 chemical bonding and molecular geometry 1 6.1 introduction chemical bonding atoms with unfilled valence shells are considered unstable. atoms will try to fill their outer shells by bonding with other atoms. chemical bond = the attractive force that holds atoms or ions together in a compound atoms form atomic bonds to become more stable. atoms become more stable by filling their valence shell or at least meeting the octet rule by getting 8 valence electrons. there are three main types of chemical bonds used by atoms to fill their valence shell: ionic covalent metallic 6.1.1 formation of ionic compounds ionic bonds are formed between metals and non-metals. ionic bonds are formed between oppositely and negative charged atoms (ions). ionic bonds are formed by the transfer of electrons. one atom loses (gives away) electrons. one atom gains (receives) electrons. use the number of valence electrons …

2 / 64

3 more for octet gains 3 e- oxidation #/ion charge of -3 6.1.2 electronic structure of cations and anions ions are formed when atoms gain or lose electrons. ions are charged atoms (positive or negative). positive ions are called cations. formed when the atom loses electrons. lose negative charge, becomes positive ion metals negative ions are call anions. formed when the atom gains electrons. gain negative charge, become negative ion non-metals drawing ionic bonds 1 – draw the lewis structure for each element. ex: na cl 2 – draw arrows to show the transfer (gain/loss) of electrons [draw extra atoms if needed] 3 – draw ion lewis diagrams showing the new charge for each ion. ex: 4- write the chemical formula for the compound formed represents the ratio of negative ions to positive ions. ex: nacl – for every 1 sodium ion, there is also 1 chlorine ion. chemical formula …

3 / 64

al electrons). single bond (2e) double bond (4e) triple bond (6e) cont… atoms can share their electrons equally or unequally. when atoms share electrons equally, it is called a non-polar covalent bond. non-polar covalent bonds form between atoms of the same type. ex: h2, cl2, when atoms share electrons unequally it is called a polar covalent bond. one atom pulls the electrons closer to itself. the atom that pulls the electrons more gets a slightly negative charge. the other atom gets a slightly positive charge. ex: water molecule bonding animation cont.., the same atoms can share both of its electron and it is called a coordinate bond or dative covalent bond. the atoms are held together because the electron pair is attracted by both of the nucleus. example. 6.2.2 polarity of covalent bonds molecular dipoles occur due to the unequal sharing of electrons between atoms in a molecule. those atoms …

4 / 64

will give you the # of bonds needed to draw the structure. 2. create a “skeleton” structure by connecting surrounding atoms to the central atom. the central atom is the one that there is one of or the least electronegative (generally the first element in the formula is the central). place electrons between the central atom and surrounding atoms so that it has an octet. (remember hydrogen only needs 2). complete octets on the outside atoms. 5. if you run out of electrons to complete the octets of the surrounding atoms, then you must move electrons from the central atom to the outside and create double or triple bonds between the central atom and a surrounding atom. 18 practice: drawing covalent bonds we can illustrate covalent bonding using lewis structures. 1 – draw a lewis structure for each element. ex: c h 2 - continue adding atoms until all atoms …

5 / 64

ired electron. nitrogen is a period 2 element and can be satisfied with less than an octet. nitrogen dioxide ………. 17 valence electrons d. expanded octet means that the central atom is sharing more than 8 electrons. third row and heavier elements can exceed the octet rule by using their empty valence d orbitals. xenon tetrafluoride xef4 24 resonance resonance refers to when more than one valid lewis structure can exist for a molecule. the actual structure lies somewhere in between the two as an average. the formal charge of an atom in a molecule is the hypothetical charge the atom would have if we could redistribute the electrons in the bonds evenly between the atoms ignoring electronegativity. you can use formal charges to identify the most reasonable lewis structure for a given molecule easy way to calculate formal charge formal charge = fc valence electrons = ve bonded pairs …

Want to read more?

Download all 64 pages for free via Telegram.

Download full file

About "chemical bonding and molecular geometry"

8.1 types of chemical bonds 6 chemical bonding and molecular geometry 1 6.1 introduction chemical bonding atoms with unfilled valence shells are considered unstable. atoms will try to fill their outer shells by bonding with other atoms. chemical bond = the attractive force that holds atoms or ions together in a compound atoms form atomic bonds to become more stable. atoms become more stable by filling their valence shell or at least meeting the octet rule by getting 8 valence electrons. there are three main types of chemical bonds used by atoms to fill their valence shell: ionic covalent metallic 6.1.1 formation of ionic compounds ionic bonds are formed between metals and non-metals. ionic bonds are formed between oppositely and …

This file contains 64 pages in PPTX format (3.7 MB). To download "chemical bonding and molecular geometry", click the Telegram button on the left.

Tags: chemical bonding and molecular … PPTX 64 pages Free download Telegram