c2b_default

Basic Chemistry

Foundation Year

Foundation Year

32
0.0 (0)
S. B.
Étudier
S. B.
This flashcard set covers fundamental concepts in chemistry at the university level, focusing on atomic structure, bonding, and chemical reactions. It delves into topics like electrons, protons, neutrons, and their roles in forming atoms and molecules, as well as the principles governing chemical bonds and reactions. The flashcards also explore different types of mixtures and the energy dynamics in chemical processes. Ideal for university students, this set provides a comprehensive overview of basic chemistry, helping learners grasp essential theories and practical examples to build a strong foundation in the subject.
Cartes-fiches
32
Utilisateurs
0
Langue
Anglais
Catégorie
Chimie
Niveau
Université
Créé / Mis à jour
26.12.2019 / 26.12.2019
  • 1  / 32

Cartes-fiches

Mixture 

Heterogeneous & homogeneous

Homogeneous

Homo = same

Uniform composition and appearance throughout

Example: Apple Juice, Air 

 

Heterogeneous

Hetero = different

Consists of visibly different substances or phases (gas,liquid,solid)

Example: Cereal in milk, soil

Suspension

Heterogeneous mixture with a solid and a liquid phase

 

Emulsion

Heterogeneous mixture with two liquids, which can't dissolve in each other 

 

exothermic

the reaction releases energy 

Example: combustion (lighting a candle)

 

endothermic

reaction absorbs energy from surroundings

Example: melting an ice cube

activation energy

the requirement of the smallest amount of energy to start a reaction OR energy amount available in a system to start a reaction

Synthesis

chemical reaction(s) which convert reactants into a product(s)

Decomposition

Breakdown of a chemical entity into two or more fragments

Composition of air (2 parts with %)

Nitrogen (78.1%)

Oxygen (20.93%)

Law of consveration of mass

In an isolated system, mass can neither be destroyed or created

Mass of products = Mass of reactants

Avogadro's number

6.02 x 1023 = 1g

 

Atomic mass number (Ar)

Total number of protons and neutrons in the nucleus (

 Atomic number 

Number of protons in the nucleus -> gives element a specific characteristic

Molecular mass (MR) 

Mass of molecule

Molar mass 

Mass of 1 mole of a substance

Rutherford's Model

Atom is mostly empty space, where electrons orbit the positive charged nucleus

Nucleus (2 things)

Protons (positively charged) & neutrons (no charge)

Isotope

Same number of protons & electrons 

Different number of neutrons 

-> Act the same but have a different atomic mass number 

 

Mass of proton

1 unit

Mass of neutron

1 unit

Cation 

positively charged ion (less electrons)

Anion

Negatively charged ion (more electrons)

Ion 

Atom or molecule with a charge (loss or gain of electrons)

Ionization Energy Ei

Minimum amount of energy required to remove the most loosely bound electron (valence electron)

Molecule 

At least two atoms bound together

Octet Rule 

Elements tend to bond to fill the most outer shell with a maximum of 8 electrons -> More stable

Partial Charge 

Stronger pull towards one element in a molecule (asymmetrical cloud) causes inequal charge distribution -> δ (Delta) is sign for partial charge

Dipole

molecule containing of two atoms with a negative and positive "pole"

Covalent bond 

Sharing of electron pairs (non-metals with non-metals)

Ionic bond

 

Donating or receiving electrons (metal with non-metal)

Étudier