Chemistry Review assignment

Determine the molar mass of H2S04

98.08

Diatomic

A molecule that contains only two atoms. All of the noninert gases occur as diatomic molecules; e. g. hydrogen, oxygen, nitrogen, fluorine, and chlorine are H2, O2, N2, F2, and Cl2, respectively.

Monatmic ion

A monatomic ion is an ion consisting of a single atom. If an ion contains more than one atom, even if these atoms are of the same element, it is called a polyatomic ion. For example, calcium carbonate consists of the monatomic ion Ca2+ and the polyatomic ion CO32-.

Nonmetal

A nonmetal is a substance that conducts heat and electricity poorly, is brittle or waxy or gaseous, and cannot be hammered into sheets or drawn into wire. Nonmetals gain electrons easily to form anions*. About 20% of the known chemical elements are nonmetals.

Molecular formula

A notation that indicates the type and number of atoms in a molecule. The molecular formula of glucose is C6H12O6, which indicates that a molecule of glucose contains 6 atoms of carbon, 12 atoms of hydrogen, and 6 atoms of oxygen.

Polyatomic bond

A polyatomic ion, also known as a molecular ion, is a charged chemical species (ion) composed of two or more atoms covalently bonded or of a metal complex that can be considered to be acting as a single unit.

Extensive property

A property that changes when the amount of matter in a sample changes. Examples are mass, volume, length, and charge.

Intensive property

A property that does not change when the amount of sample changes. Examples are density, pressure, temperature, color.

Heterogeneous mixture

A sample of matter consisting of more than one pure substance* and more than one phase*. Blood, protoplasm, milk, chocolate, smoke, and chicken soup are examples of heterogeneous mixtures.

Homogeneous mixture

A sample of matter consisting of more than one pure substance* with properties that do not vary within the sample.

Solution

A sample of matter consisting of more than one pure substance* with properties that do not vary within the sample. Also called a homogeneous mixture.

Pure substance

A sample of matter that cannot be separated into simpler components without chemical change*. Physical changes can alter the state of matter* but not the chemical identity of a pure substance. Pure substances have fixed, characteristic elemental compositions and properties.

Chemical formula

A set of chemical symbols showing the elements present in a compound and their relative proportions, and in some cases the structure of the compound.

Solid

A solid is a relatively dense, rigid state of matter, with a definite volume and shape. Molecules in solids are often packed close together in regularly repeating patterns, and vibrate around fixed positions.

Liquid

A state of matter that has a high density and is incompressible compared to a gas. Liquids take the shape of their container but do not expand to fill the container as gases do. Liquids diffuse* much more slowly than gases.

Aqueous solution

A substance dissolved in water.

Reactant

A substance that is consumed during a chemical change*.

Product

A substance that is produced during a chemical change*.

Extraction

A technique for separating components in a mixture that have different solubilities*. For example, caffeine can be separated from coffee beans by washing the beans with supercritical fluid carbon dioxide; the caffeine dissolves in the carbon dioxide but flavor compounds do not. Vanillin can be extracted from vanilla beans by shaking the beans with an organic solvent, like ethanol.

Atomic mass

A unit of mass equal to 1/12 the mass of a carbon-12 nucleus, which is 1.660 538 73 × 10-27 kg ± 0.000 000 13 × 10-27 kg [1998 CODATA values]. Abbreviated as amu or u. Sometimes called the dalton, after John Dalton, architect of the first modern atomic theory.

Accuracy

Accuracy is the correctness of a single measurement. The accuracy of a measurement is assessed by comparing the measurement with the true or accepted value, based on evidence independent of the measurement. The closeness of an average to a true value is referred to as "trueness".

Name the compound NH4Cl

Ammonium chloride

Actual yeild

Amounts of products calculated from the complete reaction of the limiting reagent is called theoretical yields, whereas the amount actually produced of a product is the actual yield. The ratio of actual yield to theoretical yield expressed in percentage is called the percentage yield.

Anion

An anion is a negatively charged ion. Nonmetals* typically form anions.

Atom

An atom is the smallest particle of an element that retains the chemical properties of the element. Atoms are electrically neutral, with a positively charged nucleus that binds one or more electrons in motion around it.

Element

An element is a substance composed of atoms with identical atomic number*. The older definition of element (an element is a pure substance that can't be decomposed chemically) was made obsolete by the discovery of isotopes*.

Metalloid

An element* with both metallic and nonmetallic properties. Examples are silicon, arsenic, and germanium.

Neutron

An elementary particle found the atomic nucleus* of all stable atoms except the hydrogen-1 atom. Neutrons have no charge and have a mass of 1.008665 daltons*.

Proton

An elementary particle found the atomic nucleus* with a positive charge equal and opposite that of the electron*. Protons have a mass of 1.007276 daltons*.

Write the formula for Carbon tetrachloride

CCL4

Write the formula for Calcium phosphate

Ca3(PO4)2

Name the compound CO

Carbon monoxide

Name the compound CsCl

Cesium chloride

Covalent compound ion

Covalent chemical bonds involve the sharing of a pair of valence electrons by two atoms, in contrast to the transfer of electrons in ionic bonds. Such bonds lead to stable molecules if they share electrons in such a way as to create a noble gas configuration for each atom.

Crystalization

Crystallization is also a chemical solid-liquid separation technique, in which mass transfer of a solute from the liquid solution to a pure solid crystalline phase occurs.

How many molecules are present in 4.6 g of H2O

1.5x10^23

An element 'E' is present as 10E and has a mass of 10.01 amu and 11E has a mass of 11.01 amu. The natural abundances of 10E and 11E are 19.78% and 80.22%. What is the average atomic mass of the element? What is the element?

10.81 amu Boron

450 Kelvin into Celsius

177C

How many significant figures are in 2200

2

How many significant figures are in 3.2 x 10^3

2

Convert 239 kg into µg

2.39x10^11

What is the correct answer in the amount of significant figures for 16.82+3.2257

20.05

Which is greater 23kg or 2300g

23Kg

What is the correct answer in the amount of significant figures for 324.6x815.991

264900

What is the correct answer in the amount of significant figures for ((3.901-3.887)÷3.901)x1.00

36x10^-3

How many significant figures are in 0.0002000

4

Convert 475 mL into kL

4.75x10-4

-230 Celsius into Kelvin

43K

How many grams of CO2 are present in one mole of CO2

44.01

200 Celsius into Kelvin

473K

How many grams of H2SO4 are present in five moles of H2SO4

490.4

How many items are present in 3 grams of NH3

4x10^23

How many significant figures are in 133.45

5

An object weighs 6.7kg and takes up 1245mL. What is the density in g/mL

5.4

Convert 5.46 mm into cm

5.46x10^-3

What is 5.6 liters converted into kiloliters

5.6x10^-3

What is 5.6 liters converted into microliters

5.6x10^6

Which is greater 50000mL or 5000L

5000L

What is 5.6 liters converted into cubic centimeters

5600

What is 5.6 liters converted into milliliters

5600

How many significant figures are in 12.0000

6

What is the correct answer in the amount of significant figures for 27÷4.148

6.5

How many significant figures are in 0.01334520

7

Derived unit

Derived units are units* constructed from the SI* system's base units*. For example, the SI unit for density is kg/m3, derived from the base units kg and m.

Name the compound N2O4

Dinitrogen tetraoxide

Distillation

Distillation is a technique for separating components of a mixture on the basis of differing boiling points. The mixture is heated, vaporizing some of the components. The vapor is collected and condensed* to isolate the components with the lowest boiling points.

Empirical formula

Empirical formulas show which elements are present in a compound, with their mole ratios indicated as subscripts. For example, the empirical formula of glucose is CH2O, which means that for every mole of carbon in the compound, there are 2 moles of hydrogen and one mole of oxygen.

Name the acid HI

Hydroiodic acid

Volatitity

In chemistry and physics, volatility is the tendency of a substance to vaporize. Volatility is directly related to a substance's vapor pressure. At a given temperature, a substance with higher vapor pressure vaporizes more readily than a substance with a lower vapor pressure.

Law of definite proportions

In chemistry, the law of definite proportions, sometimes called Proust's Law, states that a chemical compound always contains exactly the same proportion of elements by mass.

Law of conservation of mass and energy

In physics, the law of conservation of energy states that the total energy of an isolated system cannot change—it is said to be conserved over time. Energy can be neither created nor destroyed, but can change form, for instance chemical energy can be converted to kinetic energy in the explosion of a stick of dynamite.

Name the compound Fe2O3

Iron (III) oxide

Determine the following oxidation numbers or oxidation state of KClO4

K=+1 CI=+7 O=-2

Determine the following oxidation numbers or oxidation state of K2Cr2O7

K=+1 Cr=+6 O=-2

SI Unit

Le Systéme Internationale (SI) is a system of units introduced to remove barriers to international trade, based on the older metric system. It is now used in science and technical communications worldwide.

Name the compound Pbl2

Lead (II) iodide

Name the compound LiH

Lithium hydroxide

Precision

Precision is reproducibility. Saying "These measurements are precise" is the same as saying, "The same measurement was repeated several times, and the measurements were all very close to one another". Don't confuse precision with accuracy*.

Period

Rows in the periodic table* are called periods. For example, all of the elements in the second row are referred to as 'second period elements'. All elements currently known fall in the first seven periods.

Molar mass

The mass of one mole of a material. For example, the molar mass of H2O is 18.015 g (obtained by adding twice the molar mass of hydrogen to the molar mass of oxygen).

Avogadro's number

The number of particles in one mole, equal to 6.02214199 × 1023 mol-1 (± 0.00000047 mol-1)

Atomic number

The number of protons* in an atomic nucleus*. The atomic number and the element symbol* are two alternate ways to label an element. In nuclide symbols*, the atomic number is a leading subscript; for example, in 126C, the "6" is the atomic number.

Percent compostion

The percent composition of a component in a compound is the percent of the total mass of the compound that is due to that component. in the compound using the periodic table or a molecular mass calculator.

Neuclous

The positively charged central core of an atom, consisting of protons and neutrons and containing nearly all its mass.

Predicted yeild

The predicted yield is the amount that might have been expected if nothing had got lost along the way. In practice, some product will be lost during the process when purifying the product by filtration or evaporation or when transferring a liquid or when heating. Calculating percentage yield.

Limiting reactant

The reactant that limits the amount of product produced in a chemical reaction. For example, mixing one mole of H2(g) with one mole of O2 produces one mole of steam (H2O(g)), with half a mole of O2(g) remaining. The hydrogen gas limits the amount of steam produced in this case.

Molecule

The smallest particle of an element or compound that retains the chemical properties of the element or compound. A molecule is a collection of chemically bound atoms* with characteristic composition and structure. Making or breaking bonds* in a molecule changes it into a new molecule. Ionic compounds* are not composed of molecules, because there is no distinct collection of ions* that are chemically bound in the crystal.

Chemistry

The study of matter and its transformations.

Theoretical yeild

The theoretical yield of a reaction is the amount of product that would be formed if the reaction went to completion.

Mass number

The total number of protons* and neutrons* in an atom or ion. In nuclide symbols* the mass number is given as a leading superscript. In isotope* names (e. g. carbon-14, sodium-23) the mass number is the number following the element name.

Name and list the symbols of the seven diatomic elements

H2: hydrogen N2: Nitrogen O2: Oxygen F2: Florine CI2: Chlorine Br2: Bromine I2: Iodine

Write the formula for hydrosulfuric acid

H2S

Write the formula for sulfuric acid

H2SO4

Determine the following oxidation numbers or oxidation state of HNO3

H=+1 N=+5 O=-2

Determine the following oxidation numbers or oxidation state of H2O

H=+1 O=-2

Determine the following oxidation numbers or oxidation state of H2SO4

H=+1 S=+6 O=-2

Write the formula for hydrofluoric acid

HF

Write the formula for Hydrogen iodide

HI

Write the formula for nitrous acid

HNO2

Write the formula for nitric acid

HNO3

Heat

Heat is a transfer of energy that occurs when objects with different temperatures are placed into contact. Heat is a process, not a property of a material.

Name the acid HBr

Hydrobromic acid

Name the acid HCL

Hydrochloric acid

Uncertainy

...

What is the correct answer in the amount of significant figures for 7.442-7.429

0.013

Arrange from smallest to largest: 0.001187g 0.0132mg 875.2µg

0.0132mg 875.2µg 0.001187g

How many moles of carbon are present if you have 6.71 g of carbon

0.559

How many malls are present in Avogadro's number of particles

1

How many significant figures are in 0.04

1

Group

1. A substructure that imparts characteristic chemical behaviors to a molecule, for example, a carboxylic acid* group. 2. A vertical column on the periodic table, for example, the halogens*. Elements that belong to the same group usually show chemical similarities, although the element at the top of the group is usually atypical.

Binary covalent compound

A binary covalent compound is composed of two different nonmetal elements. For example, a molecule of chlorine trifluoride, ClF3 contains 1 atom of chlorine and 3 atoms of fluorine.

Binary ionic compound

A binary ionic compound is a salt consisting of only two elements in which both elements are ions, a cation (which has a positive charge) and an anion (which has a negative charge). When naming these compounds, its composition must be considered.

Cation

A cation is a positively charged ion. Metals* typically form cations.

Physical change

A change which does not transform one substance into another. For example, freezing water is a physical change because both water and ice are H2O. However, electrolysis* of water would not be a physical change because passing a strong electric current through water can decompose it into H2 and O2.

Chemical change

A chemical change is a dissociation, recombination, or rearrangement of atoms.

Chemical equation

A compact notation for describing a chemical change. The formulas of the reactants* are added together on the left hand side of the equation; the formulas of the products* are added together on the right side. Coefficients are inserted before the formulas to ensure that the equation is balanced*. The phase* in which each substance is found is usually indicated in parentheses after each formula. For example, 2 H2(g) + O2(g) = 2 H2O(g) indicates that 2 moles of hydrogen gas combine with one mole of oxygen gas to produce two moles of steam.

Compound

A compound is a material formed from elements chemically combined in definite proportions by mass. For example, water is formed from chemically bound hydrogen and oxygen. Any pure water sample contains 2 g of hydrogen for every 16 g of oxygen.

Ionic compound

A compound made of distinguishable cations* and anions*, held together by electrostatic forces.

Significant figures

A convention for recording measurements. Measurements are rounded so that they contain only the digits up to and including the first uncertain digit, when the number is written in scientific notation.

Covalent bond

A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms. The stable balance of attractive and repulsive forces between atoms when they share electrons is known as covalent bonding.

Electron

A fundamental consituent of matter, having a negative charge of 1.602 176 462 × 10-19 coulombs* ± 0.000 000 063 × 10-19 coulombs and a mass of 9.109 381 88 × 10-31 kg ± 0.000 000 72 × 10-31 kg [1998 CODATA values].

Hydrate

A hydrate is an addition compound* that contains water in weak chemical combination with another compound. For example, crystals of CuSO4·5 H2O (copper sulfate pentahydrate) are made of regularly repeating units, each containing 5 molecules of water weakly bound to a copper(II) ion and a sulfate ion.

Metal

A metal is a substance that conducts heat and electricity, is shiny and reflects many colors of light, and can be hammered into sheets or drawn into wire. Metals lose electrons easily to form cations*. About 80% of the known chemical elements are metals.

Isotope

Atoms or ions of an element with different numbers of neutrons*in their atomic nucleus*. Isotopes have the same atomic number* but different mass number*. Isotopes have very similar chemical properties but sometimes differ greatly in nuclear stability.

Chromatography

Chromatography is a method for separating mixtures based on differences in the speed at which they migrate over or through a stationary phase*.

Name the compound Cr(OH)3

Chromium (III) hydroxide

Write the formula for Cobalt (II) hydroxide

Co(OH)2

Write the formula for Iron (III) oxide

Fe2O3

Density

Mass of a substance per unit volume. Saying "the density of mercury is 13.55 g/cm3 " is the same as saying "the mass of exactly 1 cm3 of mercury is 13.55 g".

Gas

Matter in a form that has low density, is easily compressible and expandable, and expands spontaneously when placed in a larger container. Molecules in a gas move freely and are relatively far apart. "Vapor" often refers to a gas made of a substance that is usually encountered as a liquid or solid; for example, gaseous H2O is called "water vapor".

Matter

Matter is anything that has mass. Air, water, coffee, fire, human beings, and stars are matter. Light, X-rays, photons, gravitons, information, and love aren't matter.

Chemical property

Measurement of a chemical property involves a chemical change*. For example, determining the flammability of gasoline involves burning it, producing carbon dioxide and water.

Physical property

Measurement of a physical property may change the arrangement but not the structure of the molecules of a material. Examples of physical properties are density, color, boiling point, volume, temperature, and mass.

Write the formula for Dinitrogen tetroxide

N2O4

Determine the following oxidation numbers or oxidation state of NH3

N=-3 H=+1

Write the formula for Sodium bromate

NaBrO3

Write the formula for Sodium cyanide

NaCN

Write the formula for Sodium hydrogen sulfate

NaHSO4

Write the formula for Sodium iodate

NaIO3

Write the formula for sodium hydroxide

NaOH

Name the compound NH3

Nitrogen trihydride

Name the compound NI3

Nitrogen triiodide

Name the acid HNO2

Nitrous acid

Formula unit

One formula weight* of a compound.

How many protons, neutrons, and electrons are in the ion with a mass# of 31, atomic# of 15, and a Pˆ3- charge

P: 15 N: 16 E: 18

How many protons, neutrons, and electrons are in the ion with a mass# of 40, atomic# of 20, and a Caˆ2+ charge

P: 20 N: 20 E: 18

How many protons, neutrons, and electrons are in the ion with a mass# of 56, atomic# of 26, and a Feˆ3+ charge

P: 26 N: 30 E: 23

How many protons, neutrons, and electrons are in the ion with a mass# of 19, atomic# of 9, and a Fˆ1- charge

P: 9 N: 10 E: 10

Write the formula for Lead (II) nitrate

Pb(NO3)2

Name the acid H3PO4

Phosphoric acid

Name the compound PCl5

Phosphorus pentacloride

Name the compound KH2PO4

Potassium dihydrogen phosphate

Mole

SI unit for amount of substance, defined as the number of atoms in exactly 12 g of carbon-12. One mole of a molecular compound contains Avogadro's number* molecules and has a mass equal to the substance's molecular weight, in grams.

Write the formula for Tin (II) floride

SnF2

Name the compound NaC2H3O2

Sodium acetate

Name the compound NaH

Sodium hydride

Name the compound Na2SO4

Sodium sulfate

Write the formula for strontium hydroxide

Sr(OH)2

Law of multiple proportions

Statement that when two elements combine with each other to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of small whole numbers

Name the acid H2SO3

Sulfureous acid

Temperature

Temperature is an intensive property* associated with the hotness or coldness of an object. It determines the direction of spontaneous heat flow (always from hot to cold).

Name the compound P4O10

Tetraphosphorus decaoxide

Coefficient

The coefficients given before substances in a balanced chemical equation

Stoichometry

This means that it is not always possible to recover the original reaction scheme from a stoichiometry matrix. Gas stoichiometry is the quantitative relationship (ratio) between reactants and products in a chemical reaction with reactions that produce gases.