Hesi chemistry

Pregunta	Respuesta
The study of matter and its properties.	Chemistry
Everything in the universe is composed of different kinds of matter in one of its three states:	Solid, liquid, or gas
Anything that occupies space and has mass?	Matter
The scientific system of writing numbers? Composed of three parts:	Scientific method 1. mathematical sign (+ or -) 2. Significand 3. Exponential/logarithm
1. The ____ designates whether the number is positive or negative. 2. The ___ is the base value of the number or the value of the number when all values of ten are removed. 3. The ___ is a multiplier of the significant in powers of ten.	1. mathematical sign 2. significand 3. exponential/logarithm
Some calculators or other devices may write the exponent as an ___ or ___. Therefore, 3.2 x 10^5 can be written ____.	"e" or "E" 3.2 x E5
The Metric System of Measurement 1. Used to measure... 2. The basic measurements of the metric system are... 3. Each metric measurement is composed of a metric ___ and a ___ ___ of measure.	1. Length, weight, and volume 2. grams, liters, meters 3. Prefix, basic unit of measure
1. All of the prefixes are based on multiple of ___. 2. What is the acronym for the prefixes and units?	1. ten 2. king henry died unexpectedly drinking chocolate milk my giggly tanner my nana peltier family
1. Name the prefixes in order including the basic units of measure. 2. What is the order of exponentials in the prefixes	1. tera, giga, mega, kilo, hecto, deca, unit, deci, centi, milli, micro, nano, pico, femto 2. 1, 2, 3, 6, 9, 12, 15
1. A meter is a little more than ___ than a yard? 2. A dime is a little less than___? 3. A kilogram is about ___? 4. A liter is a little more than a ___?	1. Three inches longer than a yard 2. 2 cm in diameter 3. 2.2 lbs 4. quart
The three most common temperature systems are:	Fahrenheit, Celsius, and Kelvin
Fahrenheit: 1. Used in... 2. It is rarely used for any scientific measurements except for... 3. Freezing point of sea water or heavy brine at sea level? 4. Freezing point of pure water at sea level? 5. Boiling point of water at sea level? 6. Most people have a body temperature of ___ degree F/	1. United States, Jamaica, and Belize 2. body temperature 3. 0 degree F 4. 32 degree F 5. 212 degree F 6. 98.6 degree F
Celsius: 1. Sometimes called ___. 2. Freezing point of pure water at sea level? 3. Boiling point of pure water at sea level? 4. Most people have a body temp of ___.	1. Centigrade 2. 0 degree C 3. 100 degree C 4. 37 degree C
Kelvin: 1. Is only used in the ___ 2. Zero degree Kelvin is ___ and is thought to be the lowest temp achievable or absolute zero 3. The freezing point of water 4. The boiling point of water 5. Most people have a body temp of	1. scientific community 2. -273 Kelvin 3. 273 Kelvin 4. 373 Kelvin 5. 310 K
The basic building blocks of molecules?	Atoms
1. An atom's physical structure is that of a ___ and ___, sometimes called ___ ___. 2. The ___ is at the center of an atom and is composed of ___ and ___. 3. The outer most part of an atom are its orbits of ___ which spin around the nucleus at fantastic speeds, forming ___ ___.	1. nucleus, orbits, electron clouds 2. Nucleus, protons, neutrons 3. electrons, electron clouds.
1. Electrons orbit the nucleus at various energy levels called ___ or ___. 2. Atoms are most stable when an orbital is ___. 3. Most of the volume of an atom is ___.	1. shells or orbits 2. full 3. empty space
1. Protons have a ___ electrical charge. 2. Electrons have a ___ electrical charge. 3. Neutrons have ___. 4. Ground state atoms tend to have equal number of ___ and ___ making them ___ ___.	1. positive 2. negative 3. no charge at all 4. protons and electrons, electrically neutral
1. An atom that is electrically charged is called an ___ and said to be in an ___ ___. 2. Electrically charged atoms usually occur when it is in a ___ or in the form of a ___ ___.	1. ion, ionic state 2. solution, chemical compound
1. An atom in an ionic state will have lost electrons resulting in a net ___ charge or gained electrons resulting in a net ___ charge. 2. A positively charged ion 3. A negatively charged ion	1. positive, negative 2. Cation 3. Anion
1. The periodic table is made up of a series of rows called ___ and columns called ___. 2. The periodic table is a table of the known ___ rearranged according to ___. 3. Group VIII A is called the ___ ___ and has ___ charge when in a solution.	1. periods, groups 2. elements, their properties 3. noble gases, no charge
1. Groups IIIB through XIIB are called ___ ___. 2. The properties of each element can be predicted based on... 3. Two important numbers or properties of atoms that can be obtained from the periodic table are...	1. Transition metals 2. their location on the periodic chart 3. atomic number and atomic mass
1. The atomic number is the number of ___ in the ___ and defines the atom of a particular element. 2. The atomic mass of an atom is the ___ mass of each of that element. It is the sum of ___ and ___. 3. Elements with two or more structural varieties which have the same number of protons and electrons but vary in the number of neutrons.	1. protons, nucleus. 2. average, protons and neutrons 3. isotopes
1. The atomic number can be found ___ on the periodic table. 2. The atomic mass can be found ___ on the periodic table. 3. The letter in the center of the square on the periodic table...	1. at the top 2. at the bottom 3. chemical symbol
The atomic number defines the element and the number of protons. i.e. 1. If an atom has 11 protons it is... 2. If an atom has 6 protons... 3. The most common isotope of Carbon is... It has ___ and ___. 4. The isotope used for Carbon dating is ___. It has...	1. Sodium (NA) 2. Carbon (C) 3. Carbon 12, 6 protons and 6 neutrons 4. Carbon 14, 6 protons, and 8 neutrons
1. The simplest form of matter that can naturally exist in nature? It can exist as __ or ___. 2. When an element exist in combination it is called ___ and they combine in ____ ratios. 3. Recipes that contain ingredients called reactions and products.	1. Element, pure substance or in combination 2. Compound, whole number 3. Chemical equations
1. In a chemical reaction, the arrow between the reactants and the products symbolizes... 2. Mass cannot be created or destroyed during a chemical reaction =___ Therefore, once the reactants and products have been written and predicted, the equation must be ___	1. The direction of the reaction 2. Law of conservation of mass, balanced
1. Balancing the equations ensures that nothing is created or destroyed; it is simply___.	1. Rearranged
A state in chemical reactions in which reactants are forming products at the same rate that products are forming reactants.	Equilibrium
1. A reaction at equilibrium can be said to be ___. 2. What are the 4 ways to increase the reaction rate?	1. reversible 2. 1) Increase the temp of the reaction 2) increase the surface area for the reactants 3) add a catalyst 4) increase the concentrations of reactants
1. Accelerates a reaction by reducing the activation energy or the amount of energy necessary for a reaction to occur = ___. It is not used up in the reaction and can be collected on completion. 2 examples:	1. Catalyst e.i. metals and protein (enzyme)
1. A homogeneous mixture of two or more substances. 2. The part or parts that are being dissolved. 3. The part that is doing the dissolving.	1. Solution 2. Solute 3. Solvent
1. Solutions can be liquid in a ___, a solid in a ___, or a solid in a ____. 2. 4 types of solutions	1. Liquid, liquid, solid 2. Compound, Alloys, amalgams, and emulsions
Solutions: 1. Mixtures of different elements to create a single matter. 2. Solid solutions of metals to make a new one such as... 3. A specific type of alloy in which another metal is dissolved in mercury. 4. Mixtures of matter that readily separate such as water and oil.	1. Compound 2. Alloys i.e bronze is copper and tin 3. amalgams 4. Emulsions
1. Percent = _____ of the solute in the total solution. 2. A more specific way to express the concentration of a solution is in terms of its ___ ,or ___, indicated by ___. 3. A ___ of any element or compound is equal to its atomic weight or molecular weight weighed out in grams.	1. part per 100 2. Molarity, moles per liter, M 3. mole
1. One mole of any substance always contains exactly the same number of solute particles, that is, ____. This number is called____.	1. 6.02 x 10 E 23 Avogadro's number
1. Another name for an emulsion; one of its unique transformations is? 2. A heterogeneous mixture with large, often visible solutes that tend to settle out. i.e. sand and water	1. colloids, sole-gel transformation 2. suspension
1. What are the 5 main types of chemical reactions?	1. Synthesis 2. Decomposition 3. Combustion 4. Single replacement 5. Double replacement
1. A type of reaction where two elements combine to form a product. 2. The breaking of a compound into its component parts = opposite of synthesis 3. An exothermic chemical reaction usually initiated by heat acting on oxygen and a fuel compound such as hydrocarbon.	1. Synthesis 2. Decomposition 3. Combustion 4.
1. In the combustion of hydrocarbon (gas or oil), the product are... 2. Indicates an atom's outermost energy level or that portion of it containing the electrons that are chemically reactive.	1. Carbon dioxide CO2 and water H2O 2. Valence shell
Atoms are electrically ___. However, electrons can be transferred from one atom to another, and when this happens, the balance of + an - charges is lost so that charged particles called ___ are formed.	neutral ions
1. A chemical bond formed by the transfer of one or more electrons from one atom to the other. 2. In an ionic bond, the atom that gains one or more electrons, the electron acceptor, acquires a ___ charge and is called an ___.	1. Ionic bond 2. Negative; anion
1. In an ionic compound, the atom that loses electrons (the electron donor) acquires a net ___ charge and is called ___. 2. An ionic bond is generally formed between a ___. 3. An excellent example of ionic bonding is... 4. Since opposites attract, the positive cation will attract the negative anion and form an ____ bond.	1. Positive; cation 2. metal and nonmetal 3. salt 4. electrostatic
1. Formed when two atoms share electrons, generally in pairs, one from each atom. 2. Sharing of one pair of electrons; two pairs; three pairs	1. Covalent bond 2. Single, double, and triple covalent bond
1. What type of bond is the strongest of any type of chemical bond? 2. Covalent bonds are generally formed between...	1. Covalent bond 2. Two nonmetals

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