Chapter 4 : Chemical bonds

Question 1

What is an ion ?

Answer 1

Action(+) 
>Monatomic 
*Na+ Fe3+
Derive from 1 atom
>polyatomic 
*Derive from two or more atoms connected with covalent bond 
NH4/+ H3O+

Cations(-)
>Monatomic Cl- O2-
>Polyatomic NO3/- PO4/3-

Question 2

How the elemets are closes?

Answer 2

Elements close to the noble gases in the periodic table tend to gain a loose e- is in order to acheve to gain stable noble gase configuration.

Question 3

General properties of metals and non metals

Answer 3

Metals are silvery shiny solids at room temperature except one: Mercury. Metals can be mated when a metal are good conductors of heat and electrisit

Metal have low ionization energies and low e- affinities. They will form positive cations. Might be solid, liquid, gas. You cannot pound of them because they break. They do not conduct heat and electrisity well. They have high inization and electron energy.

Question 4

What is the name for 8e-?

Answer 4

called octelulmetal loose electrons, but do not become nobel gases because of neutron same as proportion.

Question 5

Isoelectromic

Answer 5

These anion are called noble gas type of ion.

Question 6

Type of ions

Answer 6

> Ion can be two types 2+ or 3+
Electrons are always removed from the orbital
Most table:noble element
2nd most stbale is when subshell has all his orbitals helpfull with orbitals =half filled subshells

Question 7

Electrostatic attraction

Answer 7

its a large number of cation, anions and anions ions arranged in a definit pattern called “crystal lattice”. Formule express only the simplest proportion of the ions in the compounds.

Question 8

Emirical formula

Answer 8

shows the simplest proportion of he atoms in the compounds.

Question 9

Ionic compounds

Answer 9

the formula is always the same as the empirical formula

the sum of the charges on the cation and anios in each formula unit must equal zero.

Question 10

Covalent bond

Answer 10

is a chemical bond in wich two or more e- are shared by 2 atoms.

Question 11

Electrons: alone or with something?

Answer 11

e- are always in pairs either in bonding pairs or membording pair .
e- alone is calld “free radical”

Question 12

Cordinate covalent bonds

Answer 12

A coordinate covalente bond is a bnd formed when one atom donates both electrons that are shared.

Question 13

Bond polarity

Answer 13

A polar covalent bond is a covalent bond ith greater e- density around one of the 2 atoms

Question 14

electronegativity

Answer 14

is the ability of an atom to attarct toward itself the electrons in a chemical bond.

Question 15

Polar or apolar?

Answer 15

Apolar, non polar is symetrical

Polar is asymetrical e- distribution electrical dipoles.

Question 16

Molecular Geometry VSEPR model

Answer 16

consider 2 things
> the polary of the covalent bond (difference in e- negativity)
>The shape of the molecule (3D shape)

Question 17

What is a shape for a molecule?

Answer 17

The shape of a molecule is determining by the number of electrons parts that surronds the central atoms.

Question 18

2e-p?

Answer 18

Cl-Be-Cl linear molecule very polar (exception)

Electronegativity difference be have as vectors, they many cancel each other.

Question 19

3e-p?

Answer 19

around the central atom=trianglar

Due to the symetrical shape its not polar as they cancel.

Question 20

4e-p?

Answer 20

tetrahedral shape

this whole molecule is non polar because they cancel due to the symetrie.

Question 21

Double and triple bond

Answer 21

occupy space only one direction. When we want to determine the hape with the usepr model, e- and multiple bonds cant as if they were single bonds

Question 22

Delocalisation e-

Answer 22

means e- to not be long strickly to 2 atoms but spreads as a cloud ever larger area.