Chemistry is hell

Cation with AI³⁺

Aluminum

Cation with NH⁺₄

Ammonium

Cation with (Ba⁺²⁾

Barium

Cation with (Cd²⁺⁾

Cadmium

Cation with (Ca²⁺⁾

Calcium

Which cation is (Cs⁺⁾

Cesium

which cation is (III) and also Chromic (Cr³⁺⁾

Chromium

which cation is (II) and cobaltous (Co²⁺⁾

Cobalt

which cation is (I) and cuprous (Cu⁺⁾

Copper

which cation is copper (II)

cupric ( Cu²⁺⁾

which cation is (H⁺⁾

Hydrogen

which cation is iron (II)

Ferrous (Fe²⁺⁾

which cation is iron (III)

ferric (Fe³⁺⁾

which cation is lead (II)

plumbous (Pb²⁺⁾

Which cation is (Li⁺⁾

Lithium

Which cation is (Mg²⁺⁾

Magnesium

Which cation is Manganese (II)

Manganous (Mn²⁺⁾

which cation is Mercury (I)

Mercurous (Hg^2+₂₎

Which cation is mercury (II)

Mercuric (Hg²⁺⁾

Which cation is (K⁺⁾

potassium

Which cation is rubidium

(Rb⁺⁾

which cation is silver

(Ag⁺⁾

Which cation is (Na⁺⁾

Sodium

which cation is Sr²⁺

strontium

Which cation is tin(II)

stannous (Sn²⁺⁾

which cation is (Zn²⁺⁾

Zinc

Which Anion is (Br^-)

Bromide

which anion is (CO^2-₃₎

Carbonate

which anion is (CIO^-₃₎

chlorate

which anion is (CI^-)

Chloride

which anion is (CrO^2-₄₎

Chromate

what anion is (CN^-)

cyanide

what anion is (Cr₂O^2-₇₎

dichromate

which anion is (H₂PO₄^-)

dihydrogen phosphate

which anion is (F^-)

fluoride

which anion is (H^-)

hydride

which anion is bicarbonate (HCO₃^-)

hydrogen carbonate

which anion is bisulfate (HSO₄^-)

hydrogen sulfate

which anion is (OH^-)

hydroxide

which anion is iodide

(I^-)

which anion is (NO₃^-)

nitrate

which anion is (N^3-)

nitride

which anion is (NO₂^-)

nitrite

which anion is (O^2-)

oxide

which anion is (MnO₄^-)

permanganate (MnO₄^-)

which anion is (O₂^2-)

peroxide

which anion is (PO₄^3-)

phospate

which anion is (SO₄^2-)

Sulfate

which anion is (S^2-)

sulfide

which anion is (SO₃^2-)

sulfite

which anion is (SCN^-)

thiocyanate

what is an anion

a negatively charged ion that forms when an atom or molecule gains one or more electrons and shows a - charge.

what is a cation

a positively charged ion that forms when an atom loses one or more electrons.and shows a + charge

what are isotopes

orms of the same chemical element that have the same number of protons but different numbers of neutrons

what is the defintion of mols in chemistry

a standard unit of measurement in chemistry used to express a specific, very large quantity of tiny particles like atoms or molecules

what is avogadro’s number and its purpose

The exact number of particles in one mole (\(6.02214076 \times 10^{23}\)) is known as Avogadro's number or the Avogadro constant.

what is atomic mass

protons+ neutrons and heavier than the atomic number

what is the atomic number

the number of protons in an element

what are intensive properties

a physical or chemical trait of matter that does not change, even if you change the size or amount of the substance

what are extensive properties

a physical or chemical measurement that changes depending on the size of the system or the amount of matter in the sample. [1]

what is the main group on the periodic table

elements in groups 1,2, 13,15,16,17,18

what is the supposed charge of elements in group 1 (Akali metals)

+1 ions by losing one valence electron

what is the supposed charge of elements in group 2 (Alkaline Earth metals)

Form +2 ions by losing two valence electrons

what is the supposed charge of elements in groups 13

Form +3 ions by losing three valence electrons.

what is the supposed charge of elements in group 14

Can share, lose, or gain to form +4 or -4 charges, though heavier elements like tin and lead can form +2 ions.

what is the supposed charge of elements in group 15

Form -3 ions by gaining three electrons to complete an octet.

what is the supposed charge of elements in group 16

Form -2 ions by gaining two electrons.

what is the supposed charge of elements in group 17 (halogens)

Form -1 ions by gaining one electron.

what is the charge of elements in group 18 (noble gases)

Carry a charge of 0 because their outer electron shells are already full.

what is the supposed charge of elements in groups 3-12

multiple variable charges (such as Iron's +2 or +3, or Copper's +1 or +2). [1, 2]

what is the equation of density (p)

mass divided by volume P= m/v

what is the equation of volume

mass/density = m/p

what is the equation for mass

density times volume = p*v

what is the molecular formula

a way of showing the exact number and type of atoms that make up a single molecule of a chemical compound

what is the empirical formula

shows the simplest whole-number ratio of elements in a compound, while a molecular formula shows the actual number of atoms of each element in a molecule

what is first step in naming molecular compounds A_bB_a

name the lst element or group

what is the second step in naming molecular compounds A_bB_a

add the suffix ide to the first part of element B

what is the third step in naming molecular compounds A_bB_a

use greek prefixes Cmono for 1, di for two, tri for 3, tetra for 4, penta for 5, hexa for 6, hepta for 7, octa for 8, nena/ennea for 9, and deca for 10) to specify the number of A and B atoms

what are the exceptions to naming molecular compounds A_bB_a

tetra reduces to tetr for oxides same for penta, hexa, etc

what ionic compounds

a neutral substance made of positively and negatively charged ions held together by strong electrostatic force and They usually form when a metal reacts with a nonmetal. [1]

• Cations and anions: The metal atom loses electrons to become a positive ion (cation). The nonmetal atom gains those electrons to become a negative ion (anion). [1]

what are molecular compounds

a chemical substance formed when nonmetal atoms share electrons to create discrete, electrically neutral molecules. [1, 2, 3]

Key Characteristics

• Covalent bonds: Atoms hold together by sharing pairs of electrons rather than transferring them.

• Composition: They typically consist of two or more different nonmetal elements (such as hydrogen, carbon, oxygen, or nitrogen).

what are polyatomic ions and which are they

charged groups of two or more atoms joined together by covalent bonds that act as a single unit and include OH^-, CH^-,CO₃^2-,SO₄^2-,SO₃^2-,NO₃^-, NO₂^-,NH₄⁺

what is the first step in naming ionic compounds A_bB_a

write down the name of the element A first

what is the second step in naming ionic compounds A_bB_a

The anion (B^b- is usually a non-metal is then named by taking the first part of the elements name and adding “ide”

How do you name polyatomic ions

they have traditional names and do not carry a ide at the end like sulfate or ion at the end.

how do you name transition metals with different oxidation numbers in different compounds

to name these compounds for the ion with the smallest charge add “ous” to the end of the name for the largest charge add “ic” to the end of the name.

what is a more reliable way to how do you name transition metals with different oxidation numbers in different compounds

is to name metals ions using roman numerals as follows Fe²⁺ —> Iron(II)

what is relative atomic mass and how do you find it

the weighted average mass of an element's atoms compared to one-twelfth of the mass of a carbon-12 atom and Multiply the mass number of each isotope by its percentage abundance.

• Add all of those values together.

• Divide the total sum by 100

ex of relative atomic mass

Example: Chlorine

• Isotope 1: Mass 35 with 75% abundance

• Isotope 2: Mass 37 with 25% abundance

• Calculation: \((35 \times 75) + (37 \times 25) = 2625 + 925 = 3550\)

• Divide by 100: \(3550 / 100 = 35.5\) [1, 2]

put in amu

what is relative molecular mass and how do you find it

the total sum of the relative atomic masses of all the atoms in a single molecule of an element or compound andHow to Find Relative Molecular Mass

To find the relative molecular mass, add up the atomic masses of all the individual atoms in the chemical formula. [1]

1. Find the chemical formula of the molecule.

2. Look up the relative atomic mass (\(A_{r}\)) for each element using a periodic table.

3. Multiply each element's atomic mass by the number of atoms of that element in the formula.

4. Add all the values together to get the final total

ex of relative molecular mass

Step-by-Step Example: Water h20

• Elements present: Hydrogen and Oxygen

• Atomic masses from the periodic table:

  • Hydrogen = \(1\)

  • Oxygen = \(16

• Number of atoms:

  • {H} = 2\) atoms

  • t{O} = 1\) atom [1]

• Calculation:

  • Atomic mass of H} \times 2) +Atomic mass of O} \times 1)\)

  • \((1 \times 2) + (16 \times 1) = 2 + 16 = 18\) [1]

in g/mol

what is stoichiometry

the calculation of the quantities of reactants and products involved in a chemical reaction