Ionic Bonds

Ionic compounds

Compounds that are composed of ions. And the ions within them are held together by ionic bonds

Ionic bonds

Electrostatic forces of attraction between oppositely charged cations and anions.

crystalline

Ionic solids have ___________ structure.

rigid, brittle

Ionic solid tends to be _____ and ______

melting, boiling

Ionic solids have higher _______ and _______ points

poor, strength, moving freely, solid

Ionic solids are ____ conductors of electricity. This is because the ________ of the ionic bonds is prevent ions from _____________ in _____ states.

easily dissolve

Most ionic solids _______________ in water.

Dissolved, melted, ions, move freely

_________ or ______ ionic compounds are excellent conductors of electricity and heat as the ____ can now ___________

soft

Sodium metal is ____ in touch

silvery-white

Sodium metal’s color is _____________.

vigorously burns

Sodium metal ________________ in the air.

explosively

Sodium metal reacts ___________ with water.

yellow-green

Chlorine gas has a ____________ color.

corrosive

Chlorine gas is extremely _________ to some metals

poisonous

Chlorine gas is extremely _________ to animals and plants

Sodium Chloride

A white crystalline compound, which is non poisonous and simply dissolves in water.

Common table salt

Another name for sodium chloride

sodium, chlorine

Sodium chloride contains ______ cations and ________ anions.

Binary ionic compounds

The compounds that are composed of only two elements. From which one element is a metal that forms a cation and the other element is a non-metal that forms an anion.

Metals

The types of elements that have a relatively low ionization potential, they tend to lose electrons quickly.

Non-metals

The types of electrons that have higher electron affinities. They readily gain electrons lost by the metals, filling their valence shells.

neutral

All substances of the ionic compounds are electrically _______.

Formula of an ionic compound

Represents the ratio of the numbers of ions in the compound, in a way that the sum of each ion’s charge gives the total answer of zero.

physical arrangement

Formula of an ionic compound does not represents its ____________________.

Isotropic forces

The attractive forces between ions that are same in all directions.

Any particular ion is attracted to all the nearby ions of the opposite charge

tightly-bound, 3D lattice structure

Isotropic forces results in the ions arranging themselves in a ____________, ___________________

Electrostatic attraction

The force that pulls opposite electric charges towards each other

769kJ

The amount of energy required to dissociate one mole of solid sodium chloride into separate gaseous Na+ and Cl- ions.

Valence electrons

Electrons in the outermost shells of the atom

Alkali metals

Name of the Group 1

Alkaline earth metals

Name for group 2

Triels

Official name for group 13

Boron group

Another name for the group 13

Tetrels

Official name of group 14

Carbon group

Another name for the group 14

Pnictogens or Pentals

Official name of group 15

Nitrogen group

Another name for the group 15

Chalcogens

The official name of the group 16

Oxygen group

Another name of the group 16

Halogens

Official name of the group 17

Fluorine group

Another name of the group 17

Group number - 10 = valence electrons

The thumb rule formula that helps us to find the number of valence electrons in Groups 13-17, for elements in period 4 and higher for most of the elements

Thallium(+3), Stannum(+4), Plumbum(+4), and Bismuth(+5)

Name the elements that are exceptions to the mentioned thumb rule

Inert pair effect

The phenomenon observed in the heavy elements of the Group 13, 14, and 15;

where the outermost s-electrons tend to remain non-bonding during chemical reactions;

This phenomenon reflects the low reactivity of the s-electron pair to participate in bonding.

Mercury

An exceptional metal in Group 12.

Unlike most metals that form single atom ions, this element can sometimes form diatomic ion

By bonding together and sharing a total +2 charge.

This element breaks the usual pattern of metals losing electrons and existing as single charged atoms.

+2 or +3

The typical cation charge that most of transition metal atoms have

Which comes from the loss of their outermost s electrons first

And then sometimes followed by the loss of 1 or 2 d electrons from the next to outermost shell.

Aufbau principle

A rule that states electrons fill atomic orbitals starting from the lowest energy level before moving to the higher ones.

In transition metals, the d orbitals are filled after the outer s orbital,

But during the ionization, the s electrons are lost first, even though they were filled earlier

Inner transition metals

The type of element that usually forms 3+ ions by losing their outermost s electrons and d or f electron during ionization.

monoatomic anions

Most _________________ when a neutral nonmetal atom gains enough electrons to completely fill its outer s and p orbitals;

thereby reaching the electron configuration of the next noble gas

Essential trace elements

Elements required by the human body in small amounts for healthy functioning.

These elements typically exist and function as ions in the body.