Naming Ionic Compounds

EXERCISE 1 : Name the following compounds:

Formula	Name	Formula	Name
a. Li2O	Lithium Oxide	n. K2O	Potassium Oxide
b. CsCl	Cesium Chloride	o. RbI	Rubidium Iodide
c. MgS	Magnesium Sulfide	p. Mg3N2	Magnesium Nitride
d. CaBr2	Calcium Bromide	q. Ca3P2	Calcium Phosphide
e. BaI2	Barium Iodide	r. Al2S3	Aluminum Sulfide
f. KH	Potassium hydride	s. Ag2O	Silver oxide
g. Na2S	Sodium sulfide	t. NaH	Sodium Hydride
h. AlN	Aluminum Nitride	u. CaO	Calcium oxide
i. AgF	Silver Fluoride	v. Na2S	Sodium Sulfide
j. ZnO	Zinc Oxide	w. LiI	Lithium Iodide
k. CdI2	Cadnium Iodide	x. CdS	cadnium Sulfide
l. BaS	Barium Sulfide	y. ZnCl2	Zinc Chloride
m. LiCl	lithium Chloride	z. CsI	Cesium Iodide

***Highlight to reveal Names

EXERCISE 2 :

What is the name for NaCl? (EXAMPLE)

sodium ion chloride ion Na1+ Cl1- sodium ion chloride ion sodium chloride NaCl

 

What is the name for Na2O? sodium ion oxide ion Na1+ O2-

What is the name for Ca3N2? calcium ion nitride ion

What is the name for NaHCO3? sodium ion bicarbonate ion

EXERCISE 3 :Name the following ionic compounds:

1)         NaBr __________________________________

2)         Sc(OH)₃ __________________________________

3)         V₂(SO₄)₃ __________________________________

4)         NH₄F __________________________________

5)         CaCO₃ __________________________________

6)         NiPO₄ __________________________________

7)         Li₂SO₃ __________________________________

8)         Zn₃P₂ __________________________________

9)         Sr(C₂H₃O₂)₂ __________________________________

10)      Cu₂O __________________________________

11)      Ag₃PO₄ __________________________________

12)      YClO₃ __________________________________

13)      SnS₂ __________________________________

14)      Ti(CN)₄ __________________________________

15)      KMnO₄ __________________________________

16)      Pb₃N₂ __________________________________

17)      CoCO₃ __________________________________

18)      CdSO₃ __________________________________

19)      Cu(NO₂)₂ __________________________________

20)      Fe(HCO₃)₂ __________________________________

EXERCISE 4 :Write the formulas for the following ionic compounds:

21)      lithium acetate __________________________________

22)      iron (II) phosphate __________________________________

23)      titanium (II) selenide __________________________________

24)      calcium bromide __________________________________

25)      gallium chloride __________________________________

26)      sodium hydride __________________________________

27)      beryllium hydroxide __________________________________

28)      zinc carbonate __________________________________

29)      manganese (VII) arsenide __________________________________

30)      copper (II) chlorate __________________________________

31)      cobalt (III) chromate __________________________________

32)      ammonium oxide __________________________________

33)      potassium hydroxide __________________________________

34)      lead (IV) sulfate __________________________________

35)      silver cyanide __________________________________

36)      vanadium (V) nitride __________________________________

37)      strontium acetate __________________________________

38)      molybdenum sulfate __________________________________

39)      platinum (II) sulfide __________________________________

40)      ammonium sulfate __________________________________

States of Matter (solids, liquids and gases) | The Chemistry Journey | F...

C2.1-E4 : Protons, Neutrons, Electrons and Isotopes

DIY MULTIPLE CHOICES  : Protons, Neutrons, Electrons and Isotopes

Exercises : 

1. Identify the number of protons, electrons, and neutrons in the following atom.

 

2. Identify the subatomic particles (protons, electrons, neutrons, and positrons) present in the following:

• 146C

• 35Cl−
  

• 24Mg2+

• 60Co

• 3H

• 40Ar

3. Given the following, identify the subatomic particles present. (The periodic table is required to solve these problems)

• Charge +1, 3 protons, mass number 6.
• Charge -2, 7 neutrons, mass number 17.
• 26 protons, 20 neutrons.
• 28 protons, mass number 62.
• 5 electrons, mass number 10.
• Charge -1, 18 electrons, mass number 36.

4. Fill in the rest of the table:

Atomic Number	Mass Number	Number of Protons	Number of Neutrons	Number of Electrons
2			2
	23			11
		15	16
	85	37
53			74

5.In the following chart, determine the number of protons, neutrons and electrons for each particular isotope. If the protons, neutrons and electrons are given, write the symbol for the isotope. (You may wish to print this page or just write your answers on a piece of paper.) 

Isotope	Protons	Neutrons	Electrons
16O
17O
137Ba
14C
	24	28	24
	9	10	9
	53	77	53
	6	7	6

6. Complete the following table

Matter (Atoms, Elements, and Compounds) - Explained

STATES OF MATTER

• Matter can exist in one of three main states: solid, liquid, or gas.
• Solid matter is composed of tightly packed particles. A solid will retain its shape; the particles are not free to move around.
• Liquid matter is made of more loosely packed particles. It will take the shape of its container. Particles can move about within a liquid, but they are packed densely enough that volume is maintained.
• Gaseous matter is composed of particles packed so loosely that it has neither a defined shape nor a defined volume. A gas can be compressed.

• liquid: A substance that flows and keeps no definite shape because its molecules are loosely packed and constantly moving. It takes the shape of its container but maintains constant volume.
• gas: A substance that can only be contained if it is fully surrounded by a container (or held together by gravitational pull); a substance whose molecules have negligible intermolecular interactions and can move freely.
• solid: A substance that retains its size and shape without a container; a substance whose molecules cannot move freely except to vibrate.

Source :https://courses.lumenlearning.com/boundless-chemistry/chapter/classification-of-matter/

Changing States Of Matter

Changing States Of Matter

Molecules can move from one physical state to another and not change their basic structure. Oxygen (O2) as a gas has the same chemical properties as liquid oxygen. The liquid state is colder and denser, but the molecules (the basic parts) are still the same. Water (H2O) is another example. A water molecule is made up of two hydrogen (H) atoms and one oxygen (O) atom. It has the same molecular structure whether it is a gas, liquid, or solid. Although its physical state may change, its chemical state remains the same.

Changes of Phase

Water vapor turning to frost is an example of deposition

There are four states of matter in the universe: plasma, gas, liquid and solid. But matter on Earth exists mostly in three distinct phases: gas, liquid and solid. A phase is a distinctive form of a substance, and matter can change among the phases. It may take extreme temperature, pressure or energy, but all matter can be changed.

There are six distinct changes of phase which happens to different substances at different temperatures. The six changes are:

• Freezing: the substance changes from a liquid to a solid.
• Melting: the substance changes back from the solid to the liquid.
• Condensation: the substance changes from a gas to a liquid.
• Vaporization: the substance changes from a liquid to a gas.
• Sublimation: the substance changes directly from a solid to a gas without going through the liquid phase.
• Deposition: the substance changes directly from a gas to a solid without going through the liquid phase.

Examples of Phase Change

I'm sure you know what most of these phases look like. Freezing is when liquid water freezes into ice cubes. Melting is when those ice cubes melt. Condensation is when dew forms on grass in the morning. Vaporization is when water boils and turns into steam. Deposition is one you may not know, but this happens when water vapor goes directly to freezing, like when there is frost on a cold winter morning. An example of sublimation happens when dry ice turns directly into gas. Gas can also change into a plasma. In order to do this you have to add an enormous amount of energy to the gas in order to free up the electrons from the atoms.

1.1 MATTER : DEFINITION AND CLASSIFICATION

Classification of Matters with Examples

Matter is a term used for everything having mass and volume. In this unit we will deal with types of matters. Pure substance, elements, compounds, mixtures are subjects of this unit.

1) Pure Matter: Same types of atoms or molecules comprise pure matters. They have some distinguishing properties. There are two pure matters, elements and compounds. Iron, alcohol, salt are examples of pure matters.

Properties of Pure Matters:

• They are homogeneous.
• They have specific physical properties like boiling point, density or freezing point.
• Temperature during phase change is constant

Now we explain pure substances one by one.

a) Elements: Element is the simplest matter which contains one type of atom. There are 109 known element in nature. We show elements with symbols like for iron we use "Fe".

Carbon "C"

Beryllium "Be"

b) Compounds: Two or more than two elements come together in specific amounts and form new matter that we call compound. Properties of compounds are totally different from elements comprising it. We show compounds with formulas like water H₂O. Ions or molecules can produce compounds.

Salt "NaCl"

Ammonia "NH₃"

Iron III Oxide "Fe₂O₃"

Properties of Compounds:

• All compounds are pure substances
• Smallest particle of compound is molecule including different types of atoms

2) Mixture: Different two or more than two types of matter (element, molecule, compound) are mixed to get mixture. All matters forming mixture keep their original properties. They are not pure matters. We can explain mixtures under two titles, homogeneous mixtures and heterogeneous mixtures.

a) Homogeneous Mixtures: All parts of mixture show same properties in homogeneous mixtures. We can call homogeneous mixtures as solutions. Salt water, sugar water, air are examples of homogeneous mixtures.

b) Heterogeneous Mixtures: Mixtures do not show same uniformity in all parts of it. In this types of mixtures, you can see different phases of matters. Water+Sand, milk, blood, soil are some common examples of heterogeneous mixtures.

Emulsion: Heterogeneous mixture including two different liquids. For example, oil-water, gasoline-water are emulsion examples.

Suspension: Heterogeneous mixture produced by one solid and one liquid matter.Sand-water, naphthalene-water are examples of suspension.

Colloids: are heterogeneous mixture type. Solute matters are homogeneously distributed in  solvent however; we can see particles of solute with naked eye or microscope in colloids but, in solutions we can not see particles with microscope. Thus; colloids are assumed to be heterogeneous mixture.

Example: Which one of the following is heterogeneous mixture?

I. Coke

II. Sea Water

III. Water+Sand

IV. Natural Gas

Coke, sea water and natural gas are homogeneous mixture but water sand is heterogeneous mixture.

Differences between Compounds and Mixtures

1. Ratio between matters forming compound is constant but ratio between matters forming mixture is variable.
2. Matters forming compounds loose their properties but matters forming mixtures preserve their properties.
3. We can decompose compounds with chemical methods but decompose mixtures with physical methods.