Chemistry Flashcards
Mass vs weight
Mass: the quantity of matter an object contains
Weight: the pull of gravity on an object of given mass
Mixture(3) vs substances(2)
Mixture
- can be separated by physical means
- 2 or more diff substances
- When mixed together, still retain it’s own qualities
Substance
- consists of 1 element
- the composition remains the same throughout
2 types of mixture and differentiate them
Homogeneous: uniformly distributed; can be separated through evaporation
Heterogeneous: visually distinguishable
Describe a solution and give an example
It consists of solute (substance being dissolved) and a solvent. Filter is not possible. Salt and water
2 types of heterogeneous and define them and give example
Colloids: filter not possible, scatter light, very dense, remain suspended
- milk, smoke, cream
Suspension: “shake well before using”; filter is possible
-blood, oil and water
What ate the 2 types of substance
Elements and Compounds
Elements vs Compounds
Elements: 1 type of atom; cannot be broken down
Compound: formed when 2 or more substances are formed chemically
Elements vs Compounds
Elements: 1 type of atom; cannot be broken down
Compound: formed when 2 or more substances are formed chemically
3 types of elements (3)
Metals: hard and shiny elements; good conductor of heat and electricity; tend to lose electrons
Nonmetals: brittle; do not conduct heat and electricity; tend to gain/share electrons
Metalloids: borderline elements between metals and non metals
3 types of compounds
Acid, base, salt
Acid(4) vs Base(4) vs Salt (3))
Acid: has sour taste, turns blue litmus to red, pH < 7, when concentrated: pH below 0
Base: turns red litmus to blue, Alkalis: strong bases, ph > 7, when concentrated: pH above 14
Salt: produced through the reaction of Base and acid; dissolves in water; conduct electricity
These are the properties that distinguish a substance from another substance. Give examples
Intrinsic
Boiling Point, acidity, sweetness, hardness, odor, length
These are properties that depend on the amount of matter observed. Give examples
Height, weight, volume, shape, temperature, and length
Formula for energy
e = mc²
Value of speed of light
3×10⁸ m/s
Endothermic vs Exothermic
Endothermic: a reaction where energy is absorbed/taken in
Exothermic: reaction resulting in the release of energy
The procedure that is used to quantitatively mix acids and bases
Titration
The reaction by which equivalent qualities of an acid and a base react ti form a salt and water
Neutralization
The tendency of liquids to dissolve in other liquids
Miscibility
The amount of solute that dissolves in a given amount of solvent to produce a saturated solution at a given temperature
Solubility
How does heat flows?
From hot body to a cold body
Celsius vs Kelvin
Celsius: + 273
Kelvin: -273
The basic building blocks of matter
Atoms
The number of protons in the nucleus of atom
Atomic number
Sum of protons and neutrons
Mass number
What do you call an atom that has the same number of protons but different number of neutrons?
Isotopes
It is the distribution of electrons in the various energy levels
Electron configuration
It is the average path that an electronic takes while traveling around the nucleus
Orbital
What is Pauli’s Exclusion Principle?
Orbitals can hold no more than 2 electrons
It is the electrons in the outermost principal energy level of an atom
Valence electrons
Attractive forces is strongest in ____ and weakest in _______
Solid, gas
This law states that the volume of a confined gas is inversely proportional to the pressure on it
Boyle’s Law
In Boyle’s Law, when volume increases, pressure ______
Decreases
This law states that the volume of a confined gas varies directly with the absolute temperature
Charles Law
The attractive force which holds together the atoms of a molecule
Chemical bond
3 kinds of chemical bonds and differentiate them
Ionic bond: transfer electrons
Covalent bond: sharing electrons
Metallic bond: electrons move freely in their valence shell
Polar covalent bond vs non polar covalent bond
Polar: unequal sharing of electrons
Non polar: equal or almost equal sharing of electrons
Avogrado’s number
6.02 × 10²³
These are the substances that undergo a chem reaction
Reactants
A type of chemical reaction wherein a single compound is formed as a result of the chemical combination of 2 elements or compounds
Composition reactions
A type of chemical reaction wherein a compound is broken down into simpler substances
Decomposition reactions
A type of chemical reaction wherein a more active element dispersed another from its chemical combination
Replacement Reactions
A type of chemical reaction where reactants exchange ions, forming two different compounds
Double replacement reactions
The property of colloidal to disperse or scatter a beam of light passing through it
Tyndall effect
The constant random motion of tiny particles suspended in a fluid caused by molecular collisions
Brownian Movement
Process by which solid attracts molecules of gas and liquid to the surface
Adsorption
