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Chemistry HL Ch 4 > Ionic Bonding > Flashcards

Ionic Bonding Flashcards

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1
Q

Define Ion

different types of ions ?

A

A charged particle

Cations ( positive ions formed by group 1,2 and 13)
Anions(neg-15,16,17)

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2
Q

Nitrate

A

NO3

-1 charge

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3
Q

hydroxide

A

OH

-1 charge

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4
Q

Carbonate

A

CO3

-2 charge

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5
Q

Hydrogen Carbonate

A

HCO3

-1 charge

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6
Q

Sulfate

A

SO4

-2 C Charge

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7
Q

Phosphate

A

PO4

-3 charge

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8
Q

Ammonium

A

NH4

(+1 Charge)

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9
Q

Describe the process of ionization

A

electrons being transferred between atoms by gaining or losing of electrons

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10
Q

Define Electrostatic Forces

A

The forces opposing charged ions are being held together by

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11
Q

Define Noble Gases

Position in Periodic table ; Chemical reactivity

A

Noble gases are inert due to having a full octet or in case of He a full shell of electrons, they are found in group 18 and are stable therefore dont react

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12
Q

What are polyatomic atoms

A

Ions made up of more than one atom which have expiriences a loss/gain of electrons

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13
Q

Ions do not form when?

A

there is isolation

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14
Q

Main forces seen in ionic bonds

A

Electrostatic forces

oppositely charges ions being attracted to each other

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15
Q

Define Ionic Lattice

A

Three Dimensial crystalline structure formed by electrostatic forces in a compound

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16
Q

What is coordination number

A

Used to express number of ions around a given ion in the lattice

17
Q

Define Lattice energy

And what it is dependent on

A

it is a measure of attraction between ions within the lattice

greater for ions that have higher charge density

18
Q

Name physical properties of ionic compounds

A
  • High melting+boiling : due to electrostatic attraction and increases with charge of ion
  • Volatility : i.e the tendency of a substance to vaporize, usually have low volatility or nonvolatile
  • Solubility : Ionic compounds in water are ‘hydrated’ , dont dissolve in non polar solutions
  • Electrical and thermal conductivity : due to free ions inside the lattice of the compound
  • Brittleness: they are brittle which is due to their crystal structure
19
Q

What is a binary compound

A

That contains only two elements having different tendencies to either gain or lose electrons

20
Q

What is a covalent bond

A

Bond betwen a non metal and a non metal which involves sharing of electrons the shared electrons are common to the two nuclei help together by electrostatic attraction

21
Q

What is the octet rule

A

refers to tendency of atoms to form a stable arrangement of eight electrons in their outer shell.

22
Q

What is Bond length

in terms of covalent bonds

A

a measure of the distance between the two bonded nuclei

23
Q

What is Bond strength

covalent bonds

A

measure of the energy required to break the bond also called bond enthalpy

24
Q

What is the general trend of bond strentgh

covalent

A

as lenghth decreases strength increases

25
Q

When is a bond polar?

A

due to difference in the electronegativities among the bonded atoms and unsymmetrical electron distribution

26
Q

Explain Dipole

A

used to indicate partially charged parts of a bond depending on electronegativity

27
Q

What is Lewis structure what does it represents

A

It is the most common way used to describe a covalent bond, it uses dots and crosses to represent the valence electrons of all atoms in a molecule.

28
Q

Coordinate Bonds within Covalent bonds

A

a case in which both the electrons come from the same atom and are being shared by a atom not contributing anything

29
Q

Explain VSEPR

VALENCE SHELL ELECTRON PAIR REPULSION

A

the geometrical shape of a molecule is dependent on the number of electrical domains it has and the number of lone pair of electrons which repel the atoms away to distort the strucutre that would be present otherwise.

Chemistry HL Ch 4 (1 decks)

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