chemistry

Question 1

What is Sodium Chloride (NaCl)?

Answer 1

A common ionic compound, its properties can be compared to other compounds to understand ionic bonding.

Question 2

Where are Noble Gases located in the periodic table?

Answer 2

Located in Group 18, characterized by their full valence shell, leading to low reactivity.

Question 3

What is Electronegativity?

Answer 3

A measure of an atom’s ability to attract electrons in a bond, crucial for understanding bond types.

Question 4

What is Core Charge?

Answer 4

The effective nuclear charge experienced by valence electrons, influencing atomic size and reactivity.

Question 5

What is Ionization Energy?

Answer 5

The energy required to remove an electron from an atom, which increases across a period due to increased nuclear charge.

Question 6

What are the Period 3 Trends?

Answer 6

As you move across Period 3, atomic size decreases, metallic character decreases, and electronegativity increases.

Question 7

What is a property of Noble Gases?

Answer 7

Low reactivity due to their complete valence shell, noble gases do not readily form compounds.

Question 8

What are some applications of Noble Gases?

Answer 8

Used in lighting (neon lights) and inert environments for chemical reactions.

Question 9

What is the historical context of Noble Gases?

Answer 9

Discovered in the late 19th century, their unique properties challenged existing theories of chemical bonding.

Question 10

What is a compound similar to Sodium Chloride (NaCl)?

Answer 10

Potassium Iodide (KI) shares ionic characteristics with NaCl, while others like ethane (C2H6) are covalent.

Question 11

What happens to Metallic Character across a period?

Answer 11

Metallic character decreases across a period, affecting the properties of elements like sodium and aluminum.

Question 12

What is Atomic Number?

Answer 12

The number of protons in an atom, defining the element.

Question 13

What is Mass Number?

Answer 13

The total number of protons and neutrons in an atom’s nucleus.

Question 14

What are Isotopes?

Answer 14

Variants of elements with the same number of protons but different numbers of neutrons, affecting atomic mass.

Question 15

How can you identify Isotopes?

Answer 15

Elements A and D are isotopes of the same element (both have 22 protons).

Question 16

What is the importance of Isotopes?

Answer 16

Used in dating techniques and medical applications.

Question 17

What is the relationship between electrons and protons in a neutral atom?

Answer 17

In a neutral atom, the number of electrons equals the number of protons, maintaining electrical neutrality.

Question 18

What is the Lewis Structure of H2O?

Answer 18

Two hydrogen atoms bonded to one oxygen atom, with two lone pairs on oxygen.

Question 19

What is the Lewis Structure of CO2?

Answer 19

Linear structure with double bonds between carbon and each oxygen.

Question 20

What is the Lewis Structure of CCl4?

Answer 20

Tetrahedral structure with single bonds between carbon and four chlorine atoms.

Question 21

What is the importance of Lewis Structures?

Answer 21

Helps in understanding molecular geometry and bonding.

Question 22

What is a unique property of Metals?

Answer 22

Metals are good conductors of electricity due to the presence of delocalized electrons.

Question 23

What are Malleability and Ductility in Metals?

Answer 23

Metals can be shaped without breaking, attributed to metallic bonding.

Question 24

What are Delocalized Electrons?

Answer 24

Electrons that are not bound to any specific atom, allowing for conductivity.

Question 25

What is the Lattice Structure in Metals?

Answer 25

Metals form a lattice of cations surrounded by a sea of delocalized electrons, contributing to their strength.

Question 26

What is Copper (II) Sulfate?

Answer 26

CuSO4, a common ionic compound used in agriculture.

Question 27

What is Calcium Hydroxide?

Answer 27

Ca(OH)2, used in various industrial processes.

Question 28

What are the properties of Ionic Compounds?

Answer 28

High melting points due to strong ionic bonds and electrical conductivity when melted or dissolved in water.

Question 29

What are the first six Alkanes?

Answer 29

Methane (CH4), Ethane (C2H6), Propane (C3H8), Butane (C4H10), Pentane (C5H12), Hexane (C6H14).

Question 30

What are the first six Alkenes?

Answer 30

Ethene (C2H4), Propene (C3H6), Butene (C4H8), Pentene (C5H10), Hexene (C6H12).

Question 31

What happens to boiling points of Alkanes and Alkenes?

Answer 31

Boiling points increase with molecular size due to greater van der Waals forces.

Question 32

What is the saturation difference between Alkenes and Alkanes?

Answer 32

Alkenes are unsaturated due to double bonds, while alkanes are saturated with single bonds.

Question 33

What are unique properties of Water?

Answer 33

Water is a polar molecule, leading to unique solvent properties.

Question 34

What is Hydrogen Bonding in Water?

Answer 34

Responsible for high boiling and melting points, as well as surface tension.

Question 35

What is the difference between Intramolecular and Intermolecular forces in Water?

Answer 35

Intramolecular bonds are within water molecules (covalent), while intermolecular bonds are between water molecules (hydrogen bonds).

Question 36

What forces must be broken for ice to melt?

Answer 36

Hydrogen bonds.

Question 37

How do you calculate % Mass of Ca in Ca(OH)2?

Answer 37

Calculation involves determining the molar mass of the compound and the mass of calcium.

Question 38

What is the formula for calculating moles?

Answer 38

Using the formula moles = mass/molar mass for given substances.

Question 39

What is involved in Empirical Formula Determination?

Answer 39

Involves converting mass to moles and simplifying the ratio.

Question 40

What is the process for writing balanced equations for chemical reactions?

Answer 40

Writing balanced equations for reactions, such as the precipitation of barium sulfate.