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2.2 Empirical Formula:
1.A formula giving the proportions of the elements present in a compound but not the actual numbers or arrangement of atoms.
2.  If the molecular formula cannot be simplified into a smaller whole-number ratio, as in the case of H2O or P2O5, then the empirical formula is also the molecular formula.
3.each element that occur in the smallest freely existing unit or molecule of the compound is expressed by the molecular formula of the compound. The molecular formula of a compound may be the empirical formula, or it may be a multiple of the empirical formula.
4. Multiply all the subscripts in the empirical formula by the whole number found in step 2. The result is the molecular formula.
5.Both have the same empirical formula, yet they are different compounds with different molecular formulas. Butene is C4H8, or four times the empirical formula; ethylene is C2H4, or twice the empirical formula.

2.3 Cation:
1.a positively charged ion, i.e. one that would be attracted to the cathode in electrolysis.
2.Ba+2
3.Cs
4.Sodium, potassium, and magnesium ions are essential for such processes as blood pressure regulation and muscle contraction.

2.4 Anion:
1.a negatively charged ion, i.e. one that would be attracted to the anode in electrolysis.
2. are formed when a nonmetal atom gains one or more electrons. Anions are so named because they are attracted to the anode (positive field) in an electric field. Atoms typically gain electrons so that they will have the electron configuration of a noble gas.
3.them form an anion with a single negative charge.
4. Monatomic anions are named by adding the suffix -ide to the stem of the name of the nonmetallic elements from which the anion is derived. For example, Cl– is called chloride and S2- is called sulfide.
5. Bromide - Br -Chloride - Cl -Fluoride - F -

2.5 Transition Metal Ions:
1.The electron configuration of transition metals is special in the sense that they can be found in numerous oxidation states.
2.Gold; Copper
3.iron commonly forms two different ions. It can sometimes lose two electrons to form the Fe2+ ion, while at other times it loses three electrons to form the Fe3+ ion.
4.The group 1 and 2 elements form cations through a simple process that involves the loss of one or more outer shell electrons. These electrons come from the s orbital and are removed very readily.
5.Titanium often used in fighter aircrafts, artificial hips and pipes in nuclear power stations. Copper because it is such a good conductor of electricity, copper is often used in electricity cables.

2.6 The Stock System of Nomenclature:
1.oxidation states of some or all of the elements in a compound are indicated in parentheses by Roman numerals.
2.The Stock system allows the specification of transition metal ionic charge when naming ionic compounds. Roman numerals are used to indicate the amount of positive charge on the cation.
3.Letters of the alphabet used in ancient Rome to represent numbers: I = 1; V = 5; X = 10; L = 50; C = 100; D = 500; M = 1000. The numbers one through ten are written I, II, III, IV, V, VI, VII, VIII, IX, and X.
4. Assign a Roman numeral to each of the following cations:
a. Sn4+=Tin(IV)
b. Fe3+=iron (III)
c. Co2+=colbaltic(IV)
d. Pb4+=Lead(IV)

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1. Gives the proportions of the elements present in a compound but not actual numbers arrangement or atoms
2. Because it is still divisible and not at its simplest form
3. Yes it can be the same
4. Divide the molar mass by empirical formula mass.
5. Carbon monoxide, butène, ethylene

2.3
1. A cation is a positively charged ion
2. Ba2+
3. Cs+
4.blood pressure regulation, bone structure, water some tees to remove harmful elements.

2.4
1. A negatively charged ion
2. Formed when a metal ions electrons and a nonmetal gains those electrons.
3. It takes less energy to gain the necessary electrons therefore forming anions.
4. They are attracted to the anode in an electric field.
5. Bromide-BR-
Chloride-CI-
Fluoride-F-
6. Combined with carions for salt, biological processes from horomone production, to DNA formation
2.5
1. Can be found in numerous oxidation states
2. 4s orbital electrons
3. Two
4. Potassium
5. Construction material, fighter aircraft electricity cables

2.6
1. Nomenclature for inorganic compounds
2. Metal ionic charge
3. Amount of positive charge of the cation
4. (IV)
-(III)
(IV)
-(IV)

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1- argon neon radon oganesson helium krypton xenon
2- they are gases In room temperature
3- the helium shell is full
4-they have 8 valence electrons
5-march 23 1962
6- they glow
Halogens
1-chlorine, CI, 35.453
Bromine, Br, 79.904
2- they are from salt
3- Ns2np5
5-find them in the earths crust

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1-Xenon, Argon, Neon, Krypton, Radon, Organesson, neon, Helium
2- they are gases that go into room temperature
3- the heliums shell is full
4- they have all had 8 vallence electrons
5- march 23 1962
6-the gasses glow

Halogens.
1- Bromine, BR, 79,904
Iodine, I, 126.90447
2- halogen means a form of salt
3- Ns2np5
4- chlorine and flourine are both gases at room temperature
5- all halogens can mainly be found inside the earths crust

Atomic Radius
1- its a way to express the size of atoms
2- its a unit of measurement of picometers
3-it generally decreases from the left to the right.
4-it then decreases to a lower group
5- the smaller sizes because of has less electrons.

ions

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1.Neon, Krypton, Helium, Argon, Oganesson, Radon, Xenon
2. They are all gases at room at room temperature
3. Because Heliums shell is full.
4. They all have 8 Valence Electrons
5. March 23, 1962
6. They all glow different colors.

Halogens
1.  fluorine, F, 18.998403
bromine, Br, 79.904
2. They are reactive nonmetallic elements that form strongly acidic compounds with hydrogen from which simple salts can be made.
3. They have characteristic outer orbit configuration of ns2 np5. The last electron during configuration occupies p orbital, hence these elements are p block elements.
4.  Bromine is a liquid, and iodine is a solid
5. The Earths Crust

Atomic Radius
1. The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding shells of electrons.
2. Angstroms (Å)
3. The atomic radius of atoms generally decreases from left to right.
4. From top to bottom down a group, electronegativity decreases.
5. Smaller in size because it has one less electron

Ion
1. They have equal numbers of protons.
2. An atom or molecule with a net electric charge due to the loss or gain of one or more electrons.
3. Those with a negative charge are called anions and those with a positive charge are called cations.
4. Ions are formed when atoms lose or gain electrons in order to fulfill the octet rule and have full outer valence electron shells.
5.

They form crystals. ...

They have higher enthalpies of fusion and vaporization than molecular compounds.

They are hard.

They are brittle.

Molecular Formula
1. The actual number of atoms for each element that is present in a compound.
2. Molecular formulas do not indicate how the atoms are arranged in the molecule.
3. The letter or letters that represent an element are called its atomic symbol.
4. Correct
5. Incorrect because its not fully a Molecular Formula.

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1. Helium, neon, argon, krypton, xenon, Radom, oganesson
2. Noble éléments are in monatomic gases at room temperature
3. There are no electrons shielding this shell from the nucleus, these two electrons, will be very difficult to move
4. They have 8 valence electrons
5. On March 23, 1962
6. The gases glow
Halogens/
1. Chlorine , CI, 35.453
Iodine, I, 126.90447
2. Halogen means salt former
3. Ns2np5
4.chlorine and fluorine are gases at room temperature
5. All halogens can be found inside the earths crust

Atomic Radius
1. A way to express the size of atoms
2. Unit of measurement are picometers
3. Generally decreases from left to right
4. Increases down a group
5. Smaller in size because it has one less electron
Ion
1. Neutral in electric charge because they have equal numbers of positive protons and negative electrons
2. When atoms gain or lose electrons
3. They’re both ions, but difference is the net electrical charge of ions
4. They’re formed when atoms lose or gain electrons
5. Form crystals, brittle and hard, conduct electricity only when dissolved In water
Molecular formula
1. Molecular formula tells us the kinds and numbers of atom present in a molecule of the compound
2. A molecular formula does not tell us about the shape of the molecule or where different atoms are
3. Subscripts tell if only one type of atom is used an is written after the symbol for that atom
4. Yes it would be correct
5. No it’s not a true molecular formula

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To clarify please answer the ALL the REVIEW Question on the bottom of each CK12 reading NOT LAST WEEKS QUESTIONS

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To clarify please answer the ALL the REVIEW Question on the bottom of each CK12 reading NOT LAST WEEKS QUESTIONS