Stage 1-2 Flashcards
Types of matter
Pure Substance and Mixtures
Matter
Everything that has mass and occupies space (has a volume)
Pure Substance
Type of matter composed by pure elements or compounds with chemical bonds. This is how they are found in nature. They have a definite composition
Element
Type of pure substance with only one type of atom.
Compound
Type of pure substance that is a chemical bond between two or more types of atoms.
Mixtures
Type of matter in which the components are physically combined. Physical combination of two or more substances that does not change the identities of the substances
Homogeneous Mixtures
Type of mixtures that is also called solution; you are not able to see the different components of the mixture because it only has one phase and a uniform composition.
Heterogeneous Mixture
Type of mixture in which you are able to see all of the different components that create the mixture.
Physical Property
They are the characteristics of things that we are able to see without affecting the identity of the substance. Ex: weight, color, boiling point, melting point, odor, luster, conductivity, state at 25 °C.
Chemical Property
Properties that indicate the ability of a substance to change into a new substance. Ex: corrosion, etc.
Physical Change
Change in which the physical appearance of a substance changes, but it’s composition stays the same. Ex: change of state, appearance, shape or size.
Chemical Change
Change in which the composition of the substance changes (the substance is turned into a new substance with new physical and chemical characteristics). A chemical reactions occurs.
Change of state
A change in which matter is converted form one state to another.
Melting point
The temperature in which a solid is converted into a liquid. Temperature in which energy is absorbed to overcome the attractive forces that hold the particles together.
Freezing point
Temperature in which a liquid changes to a solid. It is the same as the meting point. It this, temperature is lowered so energy lost and the eventually the attractive forces form a solid.
Boiling point
Point in which all the particles in a liquid gain enough energy to overcome the attractive forces between them and form a gas.
Evaporation
Formation of a gas by the escape of high-energy molecules from the surface of a liquid.
Condensation
Water vapor is turned back into a liquid as the water molecules lose energy and slow down. Course at the same temperature as the boiling point, but in this you are removing energy. Change of state of a gas to a liquid.
Sublimation
Change of state in which a solid is transforms directly into a gas without forming a liquid first.
Deposition
Th reverse process of sublimation. Change of state that is from gas state to solid state without forming a liquid.
Solid
State of matter in which the particles are tightly packed together, the particles are only able to vibrate agains each other and have a definite volume and shape. They are incompressible.
Liquid
State of matter in which the particles are able to flow, but are still close to each other. They don’t have a definite shape but they do have a definite volume.
Gas
State of matter in which particles float freely, the bounce against each other. They don’t have a definite shape nor volume (they expand until they occupy the entire container) and they are compressible. Have a lot of kinetic energy.
Period
Horizontal row of elements in the periodic table.
Group
A vertical column that contains elements that have similar physical and chemical properties.
Chemical Symbol
An abbreviation that represent the name of an element.
Representative elements
An element in the first two columns on the left of the periodic table or at the last six columns on the right (from group 1A to 8A; 1,2,13-18)
Transition elements
An element in the center of the periodic table that is designed with the letter B or is from the group numbers of 3-12.
Metals
Elements that are in he left of the heave zigzag on the periodic table. They are malleable, shiny, ductile, and good conductors of heat and electricity. They are mostly solids at room temperature.
Metalloids
Elements with properties form both non-metals and metals. They is are located along the heavy zigzag on the periodic table. They are not that malleable, futile, nor shiny; they are mostly semiconductors of heat and electricity.
Non-metals
Elements with little or no luster that are poor conducts of heat and electricity. They are located in the right of the heavy zigzag on the periodic table. They are mostly gases at room temperature.
Malleable
Ability of an element to be hammered or pressed into thin sheets or other forms, without breaking or cracking.
Ductile
Ability of an element to be turned into wires.
Binary compound
Compound formed form only two types of elements.
Ternary compound
Compound formed of three different elements.
Polyatomic compound
Compound formed of three or more elements.
Acid
Compound that a starts with H and, when dissolved in water, produces H+ (Arrhenius acids; Brønsted-Lowry acids are H+ donors and Lewis acids are election acceptors)
Base
Compound that ends in OH and, when dissolved in water, produce OH-. They are proton acceptors according to Brønsted-Lowry and electron donors according to Lewis.
Oxide
Binary compounds resulting in the mixture of Oxygen and another element (they can be metallic or nonmetallic)
Salt
Ionic bonds formed by a nonmetal and a metal (anion an action). They can be polyatomic or binary.
Valence electrons
Electrons in the outermost energy level. Electrons in the highest energy level of an atom.
Ionic bond
Bond formed between a cation and an anion after a permanent transfer of the valence electrons (for the cation tone anion). Attraction between the cation and anion.
Covalent bond
Type of bond in which valence electrons are being shared between atoms of non-metals.
Non-polar covalent
Covalent bond in which electrons are being shared easily be user he difference in electronegativities is not really big.
Polar covalent
Covalent bond in which the electrons are being share unequally because the difference in electonegativites is not really big nor small.
Ion
An atom or group of atoms that have an electrical charge because of a loss or gain of electrons.
Cation
Positively changed ion (metals that donates electrons)
Anion
Nonmetal that receives electrons and becomes the negatively charged ion.
Polyatomic ion
Group of covalently bonded non-metal atoms that have an overall charge.
Major elements
Oxygen, carbon, hydrogen and nitrogen.
Oxygen
Building block of biomolecules and water
Carbon
Budding block of organic molecules and biomolecules.
Hydrogen
Component of biomolecules, water and pH of body fluids, stomach acid.
Nitrogen
Component of proteins and nucleic acids.
Calcium
Needed for bone and teeth, muscle contraction and nerve impulses. Plastic function. Milk and dairy products.
Iron
Component of oxygen carrier hemoglobin (plastic function). Raw meat, vegetables and dried fruits. It lack is called anemia.
Phosphorus
Needs in bone and the teeth, nucleic acids and ATP. Takes part in the calcium metabolism and with the thyroid gland. It is found in fishes.
Iodine
Regulating function. Needs for property thyroid function. Sea fish, seaweed, etc.
Zinc
Antioxidant. Fish, red meat, etc. metabolic reactions, DNA synthesis, growth of borne, tissue, teeth and immune system.
Sodium and potassium
Sodium is the most abundant positive ion outside the cell and potassium is the most abundant positive ion inside the cells. They balance the liquids, and function in muscle contraction and nerve impulses. Transportation function.
Manganese
Enzymatic activation. Bone growth, blood clotting, metabolic reactions.
Molybdenum
Needs to process Fe and N, along with being a cofactor of the enzymatic system.
Selenium
Antioxidant, immune system, health of heart and pancreas.
Copper
Blood vessels, pressure, immune system and glucose tolerance.
Boron
Nutrient metabolism
Chromium
Maintenance of blood sugar levels, synthesis of biomolecules.
Magnesium
Component of bones, metabolic reaction.
Most important in the body:
oxygen and carbon
Most abundant in the universe:
Helium and Hidrogen
Most abundant earth’s crust
Silicon and oxygen.
Three greenhouse gases
CO2, CH4 (methane) and CO
Applications of copper
Plumbing and electrical wires.
Uses of silicon
Semiconductors and medicine
Petroleum (usages):
Plastics and energy sources.
Sources do emission of greenhouse gases
Industries, electrical production, machines based on fossil fuels, etc.
Physical methods to separate mixtures
Filtration, chromatography, distillation.
Chemistry
The study of matter and the changes it undergoes.
What is technology?
Practical use of scientific information.
Chemistry and biology (study of life)
Biochemistry, organic chemistry (organic compounds) and molecular biology (molecular basis of biological activity)
Chemistry and physics
Theoretical chemistry, fentochemistry.
Chemistry and agriculture
Green chemistry and agrochemistry.
Medicine and chemistry
Immunochemistry and neurochemistry
Petroleum and chemistry
Petrochemistry
Sociology
studies of human society
Physics
Study of mechanics, heat, light and other radiations
