Definitions chemistry (1)
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The document defines several key chemistry concepts: - An atom is the smallest part of an element, and a compound is made up of two or more elements joined together. Avogadro's constant is the number of particles in one mole. - Atomic number refers to the number of protons in an atom's nucleus. Mass number is the sum of protons and neutrons. Isotopes are atoms with the same number of protons but different neutrons. - Standard enthalpy changes refer to energy changes that occur during specific chemical reactions or changes of state under standard temperature and pressure conditions.
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2) The Law of Conservation of Mass says that mass is neither created nor destroyed in chemical reactions.
3) The Law of Multiple Proportions states that when two elements form more than one compound, the ratios of the masses of one element that combine with a fixed mass of the other element are ratios of small whole numbers.
4) Concepts like molar mass, the mole, and stoichiometry provide quantitative relationships between substances in chemical equations and reactions.
Basic concepts in chemistry
John Dalton proposed the first scientific atomic theory, which stated that each chemical element is composed of atoms of a single, unique type that can combine to form chemical compounds. An atom is the fundamental unit of matter and consists of a nucleus containing protons and neutrons surrounded by electrons. Atoms of the same element contain the same number of protons but can vary in the number of neutrons, resulting in different isotopes of that element. Molecules are the smallest fundamental units of compounds made of two or more atoms bonded together.
Occupational Therapy Chemical Composition of the Human Body
1) Atoms are the basic building blocks of matter and join together via chemical bonds to form molecules.
2) Molecules combine to form cells, which are the basic units of life. Cells group together to form tissues, organs, organ systems, and complete organisms.
3) The structure of an atom, including protons, neutrons, and electrons, determines its chemical properties and ability to form bonds with other atoms. Different types of bonds including covalent, ionic, hydrogen, and Van der Waals bonds influence molecular structure and function.
General Chemistry and Inorganic Pharmaceutical Chemistry Module 1 Pharmacist ...
This document provides an overview of Module 1 of the pharmacist licensure exam, which covers various topics in pharmaceutical chemistry. It will be the first module administered on the first day of the exam from 8-10 AM. The module will include questions from general chemistry, inorganic and organic medicinal chemistry, analytical chemistry, and other related chemical topics. The document emphasizes that Module 1 will be the most difficult and important module to study for. It then provides examples of key topics covered, such as atomic structure, types of chemical bonds, gas laws, and thermodynamics.
2. Atoms-56456456464655545645645644.pptx
This document discusses the structure of matter at the atomic level. It defines key terms like atoms, molecules, ions, and subatomic particles. It describes Dalton's atomic theory and the basic structure of atoms, including protons, neutrons, and electrons. It also discusses atomic number, isotopes, atomic weight, electron configuration, and the properties and uses of noble gases.
Chemistry
This document provides a summary of key chemistry concepts covered on the Regents exam, including:
1) Elements cannot be broken down chemically, while mixtures contain two or more physically combined elements or substances.
2) Chemical changes result in new substances with different properties, while physical changes do not alter the identity of the substance.
3) Gas laws relate the pressure, volume, temperature, and amount of gas in chemical reactions and problems.
4) Atoms are made up of protons, neutrons, and electrons. The number of protons determines the element.
5) Chemical bonds, including ionic and covalent bonds, result from the transfer or sharing of electrons between atoms.
Basic chemistry
Early chemists believed matter was made of four elements - air, earth, fire and water. Later, it was discovered that all matter is composed of atoms, which contain protons, neutrons and electrons. Atoms of the same element have the same number of protons but can differ in neutrons, forming isotopes. Chemical bonds form when atoms gain, lose or share electrons to achieve stable electron configurations, resulting in ionic bonds between oppositely charged ions, or covalent bonds where atoms share electrons. Chemical reactions occur when bonds are formed or broken.
Chapt02 chemistry
The document summarizes key concepts about the nature of atoms and molecules, including:
- Atoms are composed of protons, neutrons, and electrons. The number of protons determines the element.
- Electrons can be gained or lost, creating ions with positive or negative charges.
- Elements are arranged in the periodic table based on their atomic structure.
- Chemical bonds, including ionic and covalent bonds, determine how atoms combine to form molecules.
Pwpt chemistrycin
The document discusses the composition and structure of matter at the atomic and molecular levels. It defines elements as pure substances that cannot be broken down chemically, and explains that atoms are the basic units that make up elements. Atoms contain protons and neutrons in the nucleus, and electrons in energy levels surrounding the nucleus. Elements combine to form compounds with unique properties. Compounds are represented by chemical formulas showing the elements and ratios present.
Similar to Definitions chemistry (1) (20)
Occupational Therapy Chemical Composition of the Human Body
Occupational Therapy Chemical Composition of the Human Body
General Chemistry and Inorganic Pharmaceutical Chemistry Module 1 Pharmacist ...
General Chemistry and Inorganic Pharmaceutical Chemistry Module 1 Pharmacist ...
Definitions chemistry (1)
- 2. An atom is the smallest part of an element A compound is made up of two or more elements joined together Avogadro’s constant= 6.02 x 10 to power of 23 One mole is the amount of substance containing the Avogadro number of atoms, molecules or group of ions
- 3. Atomic number of an element= amount of protons in the nucleus of an element Mass number is the number of protons and neutrons in the nucleus of an atom of that isotope.
- 4. RAM - Weighted average mass - Of atom of that element - Divided by 1 twelfth - Mass of carbon 12 atom Relative Molecular Mass - average mass of - a molecule of that element - divided by 1 twelfth - The mass of a carbon 12 atom
- 5. Mass number of an isotope Is the sum of protons and neutrons In the nucleus of The atom of that isotope Relative isotopic mass: -The mass of an atom of that isotope -Divided by 1 twelfth the -Mass of a carbon 12 atom
- 6. Isotopes are atoms of the same element containing the same number of protons But different number of neutrons
- 8. 1st ionization energy: • The energy required • Per mole • To remove an electron • From the ground state of each atom • Of a mole of gaseous atoms • To create a singly positive ion
- 9. 2nd ionization energy: • The energy required • To remove an electron • From each ion • Of a mole of gaseous • Singly charged positive ion
- 11. 1st electron affinity: - Energy change when - One electron - Is added to - Each atom - In a mole - of neutral gaseous atoms
- 12. 2nd electron affinity: - Energy change when - One electron - Is added to - Each ion - In a mole of - Singly charged - Gaseous negative ions Note: second and third electron affinities are always positive numbers
- 14. Standard enthalpy of formation: - Enthalpy change when - one mole of a substance - is formed from its elements - in their standard states - under standard conditions of 1 atm pressure and at a stated temperature, usually being 298K
- 15. Standard enthalpy of reaction - Enthalpy change when - Number of moles of substances - In the equation, - As written - React under standard conditions etc
- 16. Standard enthalpy of combustion - Enthalpy change when - 1 mole of a substance - Is burned in excess oxygen - Under standard conditions - etc
- 17. Standard enthalpy of neutralisation - Enthalpy change when - 1 mole of water - Is produced by neutralization - Of a solution of an acid - By excess base - Under standard conditions etc
- 18. Standard enthalpy of atomisation (of an element) - Enthalpy change when - 1 mole of gaseous atoms - Is formed from its elements - In its standard state - Under standard conditions etc