Perrin studied the angle of deflection in positive rays.
Positive rays produce a flash on a ZnS screen.
The electron’s e/m ratio is approximately 1.7588 x 10^11 C/kg.
Plank’s quantum theory explains energy emission in a discontinuous manner.
The second orbit is 4 times away from the nucleus compared to the first orbit.
The electronic configuration of potassium (K) is [Ar]4s1.
J. Thomson proposed the existence of electrons and cathode rays.
Rise of a wetting liquid in a capillary tube is due to adhesive forces.
The magnetic quantum number (m) determines the orientation of atomic orbitals in space.
The region around the nucleus with the highest probability of finding an electron is called an orbital.
Electronic configuration of carbon-12 atom involves 18 fundamental particles.
The atomic orbits having the same energy level are referred to as degenerate orbitals.
Different wavelengths of light result in the appearance of a spectrum.
The Lyman series is produced when electrons transition to the first orbit.
The S character in the hybridization of orbital decreases with an increase in s-character.
The Heisenberg uncertainty principle states that it is impossible to know both the exact position and momentum of an electron simultaneously.
The Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers.
Orbitals are regions around the nucleus where electrons are likely to be found.
The Aufbau principle states that electrons fill the lowest energy orbitals first before moving to higher energy orbitals.
The 4d orbital is of higher energy than the 5s orbital.
Electrons in the same orbital must have opposite spins.
The atomic number of an element is determined by the number of protons in its nucleus.
The 3p orbital has a higher energy than the 4s orbital.
A cation forms when an atom loses electrons, leading to a net positive charge.
Hund’s rule states that electrons fill degenerate orbitals singly before pairing up.
The period number in the periodic table indicates the highest energy level that is being filled with electrons.
Isotopes of an element have the same number of protons but a different number of neutrons.
The atomic radius generally decreases as you move from left to right across a period in the periodic table.
Electron affinity is the energy change that occurs when an electron is added to a neutral atom to form a negative ion.
Noble gases are known for their low reactivity due to their stable electron configurations.
Ionic radii of cations are smaller than the corresponding neutral atoms, while anions are larger.
The electronegativity of elements tends to increase as you move from left to right across a period and decrease as you move down a group in the periodic table.
Metals generally have low ionization energies, making them more likely to lose electrons and form cations.
The alkali metals are located in Group 1 of the periodic table and have a tendency to lose one electron to form a +1 cation.
Transition metals are known for their variable oxidation states and often form colorful compounds.
Group 17 elements are known as halogens and readily gain one electron to form a -1 anion.
The alkali earth metals are located in Group 2 of the periodic table and have a tendency to lose two electrons to form cations with a +2 charge.
Metals are generally good conductors of heat and electricity due to their delocalized electrons.
The periodic table is organized based on the increasing atomic number of elements.
The Lanthanides and Actinides are located in the f-block of the periodic table and have electron configurations that fill the 4f and 5f orbitals, respectively.
The d-block elements are known for their variable oxidation states and are often used as catalysts in chemical reactions.
The representative elements (main group elements) in the periodic table include Groups 1, 2, and 13-18.
The noble gases are chemically inert due to their stable electron configurations, particularly the filled outer p orbitals.
The element with the atomic number 92 is uranium (U), a radioactive metal used as fuel in nuclear reactors.
The halogens are highly reactive nonmetals that readily form compounds with metals.
The element carbon (C) is unique in its ability to form a vast number of compounds due to its tetravalency and bonding versatility.
The element hydrogen (H) is the lightest and most abundant element in the universe, often forming diatomic molecules (H2).
Neon (Ne) is a noble gas located in Group 18 of the periodic table, known for its use in neon lights due to its distinctive red-orange glow.
Oxygen (O) is essential for life and is a key component of water (H2O) and many organic compounds.
The element nitrogen (N) makes up a significant portion of Earth’s atmosphere and is a crucial component of amino acids and proteins.
Sodium (Na) is an alkali metal that reacts vigorously with water to produce hydrogen gas and a basic solution.
The element chlorine (Cl) is a halogen known for its strong disinfectant properties and its use in purifying water.
Mercury (Hg) is the only metal that is liquid at room temperature and is often used in thermometers and barometers.
Copper (Cu) is a versatile metal with excellent electrical conductivity, often used in electrical wiring and plumbing.
Gold (Au) has been highly valued for its rarity and beauty throughout history and is often used in jewelry and currency.
Silicon (Si) is a semiconductor that is a key component of modern electronics, used in computer chips and solar cells.
Aluminum (Al) is a lightweight metal used in a wide range of applications, from packaging and transportation to construction.
Iron (Fe) is a crucial element in the formation of hemoglobin, the protein responsible for transporting oxygen in red blood cells.
The element uranium (U) is notable for its use in nuclear power generation and its role in nuclear weapons.
Hydrogen (H) has isotopes like deuterium and tritium, with applications in nuclear fusion and heavy water production.
The element helium (He) is lighter than air and is often used to fill balloons and airships.
Carbon (C) has several allotropes, including diamond and graphite, with varying properties and uses.
The element phosphorus (P) is essential for life and is a key component of DNA, RNA, and ATP.
Sulfur (S) is used in the production of sulfuric acid and is a key element in many amino acids and proteins.
Calcium (Ca) is an alkaline earth metal that is important for bone and teeth health, as well as nerve and muscle function.
Potassium (K) is an essential element for plant and animal cells, playing a role in nerve transmission and fluid balance.
The element iodine (I) is used in the production of thyroid hormones and is often added to table salt to prevent iodine deficiency.
The element magnesium (Mg) is an alkaline earth metal that is involved in many biochemical reactions in the body and is used in various industrial applications.
Nickel (Ni) is often used in alloys to provide corrosion resistance and heat resistance.
Titanium (Ti) is a lightweight and strong metal that is used in aerospace applications, medical implants, and sports equipment.
The element chromium (Cr) is known for its ability to form a protective oxide layer, making it useful in stainless steel and other corrosion-resistant materials.
Zinc (Zn) is often used as a coating to protect iron and steel from corrosion, and it is also essential for the functioning of enzymes in the body.
Silver (Ag) has excellent conductivity and is used in electronics, photography, and various medical applications.
Fluorine (F) is the most reactive nonmetal and is used in toothpaste and water fluoridation to prevent tooth decay.
The element bromine (Br) is the only nonmetallic element that is liquid at room temperature and is used in flame retardants and certain medical treatments.
