Extra Credit

Question 1

Element

Answer 1

An substance consisting of only one type of atom, meaning it cannot be broken down into a simpler substance by ordinary chemical processes.

Examples of elements: Hydrogen, Oxygen, Carbon, Silver. Elements can be found on the periodic table.

Question 2

Neutron

Answer 2

A subatomic particle that is found in the nucleus of every atom, except that of simple hydrogen.

The particle has no electrical charge, meaning it is neutral.

Question 3

Compound

Answer 3

A substance that has two or more chemical elements whose atoms are bonded together.

Examples of compounds: water, salt, sugar, baking soda, and alcohol.

Question 4

Proton

Answer 4

A positively charged subatomic particle in an atom.

Example of protons is the single proton in the nucleus of a hydrogen atom.

Question 5

Inorganic

Answer 5

A compound that does not contain carbon-hydrogen bonds.

Example: Table salt, sapphire, sulfuric acid.

Question 6

mass number

Answer 6

The total number of protons and neutrons in a nucleus.

Example : Helium , 2 protons & 2 neutrons, for a mass number of 4.

Question 7

Isotope

Answer 7

An atom of an element that has a different number of neutrons than the standard.

Example : Carbon-13, which contains 6 protons and 7 neutrons, as opposed to C, which contains 6 protons and 6 neutrons.

Question 8

Solute

Answer 8

A substance that is dissolved in a solvent.

Example : Salt (solute) being dissolved in water.

Question 9

Suspension

Answer 9

A heterogeneous mixture of a fluid and solid particles.

Example : the mixture of chalk and water, the mixture of flour and water.

Question 10

Catalyst

Answer 10

A substance that speeds up a chemical reaction, but is not consumed by the reaction itself.

Example : can include enzymes and elements such as platinum and iridium, as well as an acid-base.

Question 11

Base

Answer 11

A substance that can neutralize the acid by reacting with hydrogen ions.

Example : caustic soda, limewater.

Question 12

Salt

Answer 12

An ionic compound formed from reaction of an acid with a base.

Example : sodium chloride, potassium dichromate, calcium chloride.

Question 13

Mole

Answer 13

The amount of a substance whose mass in grams is numerically equal to its molecular or formula weight.

Example : one mole of carbon-12 atoms has 6.02214076 × 10^23 atoms and a mass of 12 grams

Question 14

Isomer

Answer 14

Compounds with the same molecular formula but different structures.

Example : C3H7OH ; propan-1-ol (n-propyl alcohol; I) and propan-2-ol (isopropyl alcohol; II)

Question 15

Atom

Answer 15

The smallest and simplest particle of an element.

Example : Neon (Ne), Hydrogen (H)

Question 16

Electron

Answer 16

A negatively charged subatomic particle.

Example : uranium atom has 92 electrons

Question 17

molecule

Answer 17

A group of atoms held together by covalent bonds.

Example : H2O (water), N2 (nitrogen), O3 (ozone)

Question 18

Ionic

Answer 18

Something carrying a net electrical charge.

Ex: as an ionic bond or ionic compound.

Question 19

Organic

Answer 19

Concerned with carbon and especially carbon compounds which are found in living things.

Example : Nucleic acids, fats, sugars, proteins, enzymes.

Question 20

atomic weight

Answer 20

The weighted average mass of an element’s atoms.

Example : atomic weight of helium is 4.002602

Question 21

Mixture

Answer 21

A blend of two or more substances, each of which retains its chemical identity.

Example : homogenous (steel , rain) and heterogenous (cereal in milk, ice in soda) mixtures.

Question 22

Solution

Answer 22

A homogeneous mixture that contains particles the size of a typical ion or small molecule.

Examples : salt water, rubbing alcohol, and sugar dissolved in water.

Question 23

Solvent

Answer 23

The substance in which another substance (the solute) is dissolved.

Example : water, ethanol, toluene, chloroform, aceton.

Question 24

Acid

Answer 24

A substance that provides H+ ions in water.

Examples : sulfuric acid, nitric acid, hydrochloric acid, citric acid and acetic acid.

Question 25

Buffer

Answer 25

A combination of substances that act together to prevent a drastic change in pH; usually a weak acid and its conjugate base. Examples : A acid based buffer is acetic acid (CH3COOH) and sodium acetate (CH3COONa). A base buffer is made of ammonia (NH3) and ammonium chloride (NH4Cl).

Question 26

Enzyme

Answer 26

A protein or other molecule that acts as a catalyst for a biological reaction. Examples : Lipases, Amylase, Maltase, and Trypsin.

Question 27

Molarity

Answer 27

Concentration expressed as the number of moles of solute per liter of solution. Examples : M = n/v or M = mol solute / L of Solution

Question 28

pH

Answer 28

A measure of the acid strength of a solution; the negative common logarithm of the H3O+ concentration. Examples : on the pH scale, lemon juice has a 2, black coffee a 5, pure water a 7, hand soap a 10, and bleach a 12.

Question 29

functional group

Answer 29

An atom or group of atoms within a molecule that has a characteristic structure and chemical behavior. Examples : some groups include Aldehydes, Ketone, Amine, Amino , Amide, and Ethers.

Question 30

electron shell

Answer 30

A grouping of electrons in an atom according to energy.

Question 31

atomic number

Answer 31

The number of protons in the nucleus of an atom of a given element. Example : Cl = 17, O = 8, H = 1

Question 32

chemical bond

Answer 32

A lasting attraction between atoms, ions or molecules that enables the formation of chemical compounds. Examples : ionic bonds, covalent bonds, hydrogen bonding.

Question 33

ionic bond

Answer 33

The electrical attractions between ions of opposite charge in an ionic compound. Typically formed between one metallic and one nonmetallic atom. Example : LiF - Lithium Fluoride, NaBr - Sodium Bromide.

Question 34

covalent bond

Answer 34

A bond formed by sharing electrons between atoms. Examples : water, diamonds, H2

Question 35

exergonic reaction

Answer 35

A spontaneous reaction or process that releases free energy and has a negative ∆G. Example : cellular respiration C6H12O6 (glucose) + 6 O2 -> 6 CO2 + 6 H2O this reaction release energy which is used for cell activities.

Question 36

endergonic reaction

Answer 36

A nonspontaneous reaction or process that absorbs free energy and has a positive ∆G. Example : photosynthesis and the melting of ice into liquid water.

Question 37

activation energy

Answer 37

The amount of energy necessary for a reaction to occur; it determines the reaction rate. Example : activation energy is needed to start a car engine, turning the key causes a spark that activates the burning of gasoline in the engine.

Question 38

metric measurements

Answer 38

Unit of measurements used for mass, length, volume, temperature, and time. Example : SI units (kg, m, m3, K, s) , and English units (in, ft, oz, lbs.)

Question 39

synthesis reactions

Answer 39

A type of reaction in which multiple reactants combine to form a single product. Examples: Water: 2 H2(g) + O2(g) → 2 H2O(g) Carbon dioxide: 2 CO(g) + O2(g) → 2CO2(g) Ammonia: 3 H2(g) + N2(g) → 2 NH3(g)

Question 40

decomposition reactions

Answer 40

A type of chemical reaction in which one reactant yields two or more products. Examples : AB → A + B

Question 41

neutralization reactions

Answer 41

A type of chemical reaction in which a strong acid and strong base react with each other to form water and salt. Example : when Sodium hydroxide is added to hydrochloric acid. Sodium chloride and water are formed

Question 42

redox reactions

Answer 42

A type of chemical reaction that involves a transfer of electrons between two species. Example : formation of hydrogen fluoride

Question 43

% solution

Answer 43

An amount or volume of chemical or compound per 100 mL of a solution. Example : 1 gram of sodium chloride, brought to a final volume of 100 ml with distilled water, is a 1% NaCl solution.