Chemistry - Mr Larry - Final Notes

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ammonium carbonate

(NH₄)₂CO₃

high

*describe this property in an ionic compound* boiling point

brittle

*describe this property in an ionic compound* brittleness

good

*describe this property in an ionic compound* electrical conductivity in the liquid state

poor

*describe this property in an ionic compound* electrical conductivity in the solid state

good

*describe this property in an ionic compound* electrical conductivity when dissolved in water

hard

*describe this property in an ionic compound* hardness

high

*describe this property in an ionic compound* melting point

no

*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* a drinking glass breaks into smaller pieces

no

*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* a piece of ice melts

yes

*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* a tomato smells rotten

yes

*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* baking powder produces a gas that makes a cake rise

yes

*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* candle wax burns

yes

*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* drain cleaner is mixed with water and the solution becomes warm

yes

*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* green leaves turn yellow and red as the seasons change

no

*for each statement, write yes if evidence of a chemical reaction is present. write no if there is no evidence of a chemical reaction* molten candle wax solidifies

Cs₂SO₄(l) + H₂O(l) (water)

*predict the products for each reaction. write the formulas for these products on the product side of each equation. then indicate what type of product is produced during the reaction shown in precipitates* CsOH(aq) + H₂SO₄(aq) → ___+____

KBr + H₂O (water)

*predict the products for each reaction. write the formulas for these products on the product side of each equation. then indicate what type of product is produced during the reaction shown in precipitates* HBr(aq) + KOH(aq) → ___ + ___

2KCl(g) + H₂S(g) (gas)

*predict the products for each reaction. write the formulas for these products on the product side of each equation. then indicate what type of product is produced during the reaction shown in precipitates* K₂S(aq) + HCl(aq) → __+__

Exothermic

- gas to liquid to solid - energy is released - bomb - burning anything - making ice cream - anything that emits light

ionic

- nonmetal/metal - transfers electrons - has polyatomic - has roman numerals

covalent

- shares electrons - nonmetal/nonmetal - uses prefixes - double covalent bond - 4

Endothermic

- solid to liquid to gas - energy taken in - snow melting - baking anything (bread) - water/perspiration evaporates

synthesis reaction

2 or more substances -> 1 compound

Hydrate

A compound that has a specific number of water molecules bound to its atoms

Period

A horizontal row of elements in the modern periodic table; series

anion

A negatively charged ion

silver nitrate

AgNO₃

Transition elements

An element in groups 3-12 of the modern periodic table and further divided into transition metals and inner transition metals

Electrolyte

An ionic compound whose aqueous solution conducts an electric current

bromine chloride

BrCl

methane

CH₄

carbon monoxide

CO

carbon dioxide

CO₂

calcium oxalate

CaC₂O₄

calcium hydride

CaH₂

chlorine trifluoride

ClF₃

chromium(II) hydroxide

Cr(OH)₂

2, 2

Cu(NO₃)₂(aq) + __ NaOH(aq) → Cu(OH)₂(s) + __ NaNO₃(aq)

copper(I) chloride

CuCl

5, 3, 4

C₃H₈(g) + __ O₂(g) →__ CO₂(g) + __ H₂O(g)

iron(II) nitrate

Fe(NO₃)₂

fluorine

F₂

(g)

Gas

Alkali metal

Group 1 elements, except for hydrogen, they are reactive and usually exist as compounds with other elements

hydrobromic acid

HBr

bromic acid

HBrO₃

nitrous acid

HNO₂

nitric acid

HNO₃

mercury(II) nitrate

Hg(NO₃)₂

mercury(I) chloride

Hg₂Cl₂

carbonic acid

H₂CO₃

bent

H₂O

water

H₂O

3, 3

H₃PO₄(aq) + __ KOH(aq) → __ H₂O(l) + K₃PO₄(aq)

potassium cyanide

KCN

potassium sodium carbonate

KNaCO₃

lithium acetate

LiCH₃COO

(l)

Liquid

magnesium hydroxide

Mg(OH)₂

nitrogen trichloride

NCl₃

nitrogen trifluoride

NF₃

ammonia

NH₃

amonia

NH₃

ammonium acetate

NH₄CH₃COO

nitrogen monoxide

NO

sodium dihydrogen phosphate

NaH₂PO₄

sodium phosphate

Na₃PO₄

trigonal bipyramidal

NbBr₅

nickel(II) nitrate

Ni(NO₃)₂

dinitrogen tetroxide

N₂O₄

oxygen dibromide

OBr₂

lead (II) chloride

PbCl₂

diphosphorus pentoxide

P₂O₅

single-replacement reaction

Q + XZ → X + QZ

synthesis reaction

Q + Z → QZ

double replacement reaction

QT + XZ → QZ + XT

decomposition reaction

QT → Q + T

sulfur tetrachloride

SCl₄

Selenium tetrachloride

SeCl₄

tin(IV) nitrate

Sn(NO₃)₄

(s)

Solid

strontium nitrate

Sr(NO₃)₂

16, 8

S₈(s) + ___ Cu(s) → ___ Cu₂S(s)

tellurium tetrabromide

TeBr₄

tellurium diiodide

TeI₂

Formula unit

The simplest ratio of ions represented in an ionic compound

Group

Vertical column of elements in the periodic table; arranged by increasing atomic number; families

(aq)

Water solution

zinc chlorate

Zn(ClO₃)₂

2, 2

__ SO₂(g) + O₂(g) → __ SO₃(g)

2, 3, 2

___ Al(s) + ____ Cl₂(g) → ___ AlCl₃

ionic

___ compounds are generally composed of a metal and a nonmetal

nitrate

___ is an example of an ion that forms resonance structures (more than one structural formula)

Crystal lattice

a 3-dimensional geometric arrangement of particles in which each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions; vary in shape due to sizes and relative numbers of the ions bonded

anion

a Cl⁻ ion is an example of a ____

binary compound

a ___ contains only two elements

subscript

a ___ is a small number used to represent the number of ions of a given element in a chemical formula

structural formula

a ___ shows the arrangement of the atoms in a molecule

Pi bond

a bond that is formed when parallel orbitals overlap to share electrons

Covalent bond

a bond that results from the sharing of valence electrons

Synthesis reaction

a chemical reaction in which two or more substances react to yield a single product

Endothermic

a chemical reaction or process in which a greater amount of energy is required to break the existing bonds in the reactants than is released when the new bonds form in the product molecules

Exothermic

a chemical reaction or process in which more energy is released than is required to break bonds in the initial reactants

Double replacement reaction

a chemical reaction that involves the exchange of ions between two compounds and produces either a precipitate, a gas, or water ex) compound + compound -> 1-2 compounds

Decomposition reaction

a chemical reaction that occurs when a single compound breaks down into two or more elements or new compounds

Single replacement reaction

a chemical reaction that occurs when the atoms of one element replace the atoms of another element in a compound

ionic bond

a force that holds together atoms that are oppositely charged

Halogen

a highly reactive group 17 element

Alloy

a mixture of elements that has metallic properties; most commonly forms when the elements are either similar in size (substitutional alloy) or the atoms of one element are much smaller then the atoms of another (interstitial)

Lewis structure

a model that uses electron-dot structures to show how electrons are arranged in molecules. pairs of dots or lines represent bonding pairs

VSEPR (valence shell electron pair repulsion) model

a model used to determine molecular shape

Structural formula

a molecular model that uses symbols and bonds to show relative positions of atoms; can be predicted for many molecules by drawing the Lewis structure

monatomic

a one-atom ion is called a ___ ion

Oxyanion

a polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms

cation

a positively charged ion is called a ___

Hybridization

a process in which atomic orbitals are mixed to form new, identical hybrid orbitals

Precipitate

a solid produced during a chemical reaction in a solution

Aqueous solution

a solution in which the solvent is water

Reactant

a starting substance in a chemical reaction

Chemical equation

a statement using chemical formulas to describe the identities and relative amounts of the reactants and products involved in the chemical reaction ex) 2 Fe(s) + 3Cl₂(g) -> 2FeCl₃ (s)

Product

a substance that forms in a chemical reaction

Polar covalent bond

a type of bond that forms when electrons are not shared equally

Inner transition metal

a type of group B element that is contained in the f-block of the beriodic table and is characterized by a filled outermost orbital and filled or partially filled 4f and 5f orbitals

activity

ability of an element to react

salt + water NaCl + H₂O

acid + base → ___+___ HCl + NaOH →___+___

metallic oxide + water SO₃ + H₂O

acid →___+___ H₂SO₄ →___ +___

metal compound + hydrogen MgCl₂ + H₂

active metal + acid → ___+___ Mg + 2HCl

Al(NO₃)₃

aluminum nitrate

(NH₄)₂Cr₂O₇

ammonium dichromate

Bond dissociation

amount of energy to break a specific bond (hydrogen is the easiest bond to break)

Ion

an atom or bonded group of atoms with a positive or negative charge

Metal

an element that is solid at room temperature, a good conductor of heat and electricity, and generally is shiny; most metals are ductile and malleable

Noble gas

an extremely unreactive group 18 element

Anion

an ion with a negative charge

Cation

an ion with a positive charge

Net ionic equation

an ionic equation that includes only the particles that participate in the reaction

Complete ionic equation

an ionic equation that shows all the particles in a solution as they realistically exist

Oxyacid

any acid that contains hydrogen and an oxyanion (any acid that contains oxygen) ex.) H₂SO₄

BaBr₂

barium bromide

the nuclei of two attached atoms

bond length is the distance between ____

CdSO₄

cadmium sulfate

Ca + H₂O → CaO + H₂

calcium and water

CaBr₂

calcium bromide

CaO

calcium oxide

CS₂

carbon disulfide

CI₄

carbon tetraiodide

Polyatomic ion

charged particle containing more than one atom

Monatomic ion

charged particle containing only one atom

Periodic law

chart that organizes all known elements into a grid of horizontial rows (periods), and vertical columns (groups/families) arranged by increasing atomic number

catalyst

chemical formula written over the arrow in a chemical equation signifies a ___ for the reaction

CrBr₃

chromium(III) bromide

metal + oxygen → metal oxide nonmetal + oxygen → nonmetal oxide compound + oxygen → 2 or more oxides CH₄ + 2O₂ → CO₂ + 2H₂O S + O₂ → SO₂

combustion reaction

Ionic compound

compounds that contain ionic bonds

Resonance

condition that occurs when more than one valid Lewis structure exists for the same molecule

electrolysis

decomposition of a substance by an electric current (separates elements)

one compound → 2 or more elements and/or compounds AB → A + B 2H₂O → 2H₂ + O₂ AX → A + X

decomposition reaction

H₂ N₂ O₂ F₂ Cl₂ Br₂ I₂

diatomic elements

C₂Cl₆

dicarbon hexachloride

N₂S₃

dinitrogen trisulfide

Si₂Br₆

disilicon hexabromide

2 compounds → 2 different compounds AX + BY → AY + BX NaOH + HCl → NaCl + H₂O Pb(NO₃)₂ + 2KI → PbI₂ + 2KNO₃

double replacement reaction

Sigma bond

electrons are shared in an area centered between two atoms

Transition metal

element in groups 3-12 that is contained in the d-block of the periodic table and, with some exceptions, is characterized by a filled outermost s orbital of energy level n, and filled or partially filled d orbitals of energy

Metalloid

element that has physical and chemical properties of both metals and nonmetals

Representative elements

elements designed with an A; from groups 1, 2, and 13-18 in the modern periodic table, possessing a wide range of chemical and physical properties

noble gas

elements tend to react so that they acquire the electron structure of a ___

Cl, Se, Ar, etc

elements that are anions

Na, Mg, Li, etc

elements that are cations

Nonmetal

elements that are generally gases or dull, brittle solids that are poor conductors of heat and electricity

Ionization

energy to remove electrons (nobel gases highest)

double replacement reaction

exchange of (+) ions between 2 compounds and produces a precipitate, gas, or water

F₂ + 2KI → I₂ + 2KF

fluorine and potassium iodide

Oxidation number

for a monatomic ion, is equal to the change

hydro-

for binary acids, the hydrogen part of the compound is named using the prefix ___

Interstitial alloy

formed when the small holes in a metallic crystal are filled with smaller atoms (carbon steel)

Coordinate covalent bond

forms when one atom donates a pair of electrons to be shared with an atom or ion that needs two electrons to become stable (both electrons share)

Molecule

forms when two or more atoms covalently bond and is lower in potential energy than its constituent atoms

Empirical formula

formula that shows the smallest whole-number mole ratio of elements in a compound

Alkaline earth metal

group 2 elements in the modern periodic table and are highly reactive

Substitutional alloy

has atoms of the original metallic solid replaced by other metal atoms of similar size (sterling silver and 12 carat gold)

4 bonds

how many bonds does the carbon family have

1 bond

how many bonds does the halogen family have

3 bonds

how many bonds does the nitrogen family have

2 bonds

how many bonds does the oxygen family have

four

how many electrons are shared in a double covalent bond?

2 elements

how many elements does a binary elements?

1 (2,3,4,5,6,7)

how many valence electrons does group 1 have (group 2, 13,14,15,16,halogens?)

HBr

hydrobromic acid

HCl

hydrogen chloride

e⁻

if __ is under the arrow in an equation, it is electrolysis

one

if no number appears in the subscript place, the assumption is that the number equals ____

oxyanion

if such an ion is negatively charged and includes one or more oxygen atoms, it is called a ___

sigma bond

if the electrons shared are centered between the two atoms, the attachment is called a ___

-ic

if the name of the anion of an oxyacid ends in -ate, the acid name contains the suffix ___

pi bond

if the sharing involves the overlap of parallel orbitals, the attachment is called a ___

-ate

if two such ions can be formed that contain different numbers of oxygen atoms, the name for the ion with more oxygen atoms ends with the suffix ___

heat

if___ is over the arrow in an equation, reactants are heated

Combustion reaction

in a chemical, the number written in front of reactants with oxygen, releasing energy in the form of heat and light ex) the -> in a chemical equation

zero

in ionic compounds, the sum of the charges of all the ions equals to ___

terminal atom

in molecules, hydrogen is always a ___ (atom on the end)

mono-

in naming the first element in a formula, the prefix ___ is not used

cation; anion

in the chemical formula for any ionic compound, the chemical symbol for the ___ is written first, followed by the chemical symbol for the ___

Coefficient

in the chemical, the number written in front of a reactant or product, in the balanced equation describes the lowest whole number ratio of the amounts of all reactants and products ex) 2 in 2Fe(s)

32; 6(S) + 24(O) = 30 + 2 = 32

in the sulfate ion (SO₄²⁻), ___ electrons are available for bonding

as molecules containing two atoms

in what form do elements such as hydrogen, nitrogen, and oxygen normally occur?

Electronegativity

indicates the relative ability of an element's atoms to attract electrons in a chemical bond

Spectator ion

ion that does not participate in a reaction

polyatomic

ions made up of more than one atom are called ___ ions

negative

ions that have larger charges tend to produce a more ___ lattice energy than ions with smaller charges do

Fe(OH)₂

iron(II) hydroxide

FeBr₃

iron(III) bromide

less

large ions tend to produce a ___ negative value for lattice energy than smaller ions do

Pb₃(PO₄)₂

lead(II) phosphate

activity series

list of elements arranged according to the ease with which they undergo certain chemical reactions

LiF

lithium fluoride

Li₂S

lithium sulfide

MgBr₂ + Cl₂ → MgCl₂ + Br₂

magnesium bromide and chlorine

Mn₂O₇

manganese(VII) oxide

HgBr₂

mercury (II) bromide

salt 2KCl

metal + halogen →___ 2K + Cl₂ →___

metal oxide + carbon dioxide MgO + CO₂

metallic carbonate →____ +____ MgCO₃ → ___+___

metal chloride + oxygen 2NaCl + 3O₂

metallic chlorate → ___ + ___ 2NaClO₃ → ___+___

metal oxide + water CaO + H₂O

metallic hydroxide →___+___ Ca(OH)₂ →___+___

octet

most of these elements have a set of eight outermost electrons, which is called a stable ___

Salts

name for most ionic compounds other than oxides

gaining

nonmetals form a stable outer electron configuration by ___ electrons and becoming anions

combustion reaction

occurs when a substance reacts with oxygen, releasing energy in the form of heat and light

single-replacement reaction

one element replaces another element in a compound

Solute

one or more substances dissolved in a solution ex.) sugar/salt in water

Percent composition

percent of mass by each element in a compound

6K + Al₂O₃ → 2Al + 3K₂O

potassium and aluminum oxide

K₃PO₄

potssium phosphate

reactant type: single replacement

reactants: an element and a compound products: an element and a compound

reactant type: decomposition

reactants: one products: two or more

reactant type: combustion

reactants: one plus oxygen products: one or more oxides

reactant type: double replacement

reactants: two compounds products: two compounds

reactant type: synthesis

reactants: two or more products: one

Electron sea model

represents the way electrons exist in metals

valid lewis structure

resonance occurs when more than one ____ can be written for a molecule

(+)

separates 2 or more reactants/products

->

separates the reactants from products

AgCH₃COO

silver acetate

Ag₂O

silver oxide

decomposition reaction

single compound breaks down into 2 or more elements or compounds

A + BX → AX + B metal + compound → new compound and the replaced metal nonmetal + compound → new compound and the replaced nonmetal 2HCl + Zn → ZnCl₂ + H₂ Mg + 2HCl → H₂ + MgCl₂ MgBr₂ + Cl₂ → MgCl₂ + Br₂

single-replacement reaction

Na₂CO₃

sodium carbonate

Octet rule

states atoms lose, gain, or share electrons in order to acquire the stable electron configuration of a noble gas; 8; 8 electrons

Sr(NO₃)₂

strontium nitrate

lower right

subscripts are written to the __ of the symbol for the element

nucleus electrons ions

such an attachment may form by the attraction of the positively charged ____ of one atom for the negatively charged ___ of another atom, or by the attraction of charged atoms, which are called ____

SO

sulfur monoxide

H₂SO₃

sulfurous acid

A + B → AB 2Mg + O₂ → 2MgO 2H₂ + O₂ → 2H₂O

synthesis reaction

false; some of them are, some turn into long pairs

t/f all electrons in an atom are available for bonding

false; they are not

t/f the electrons in a coordinate covalent bond are donated by both the bonded atoms

TeCl₄

tellurium tetrachloride

noble gases

the ___ are a family of elements that have very little tendency to react

lattice energy

the ___ is the energy required to separate the ions of an ionic compound

crystal lattice

the ____ of ionic compounds affects their melting and boiling points

Metallic bond

the attraction of a metallic cation for delocalized electrons

valence energy level

the attractions may also involve ___ electrons, which are the electrons in the outermost ____

two

the carbon dioxide molecule contains ___ double bonds

lowest

the central atom in a molecule is the one with the ____ electron affinity

oxidation number electrons

the charge of such an ion is equal to the atom's ___, which is the number of ___ transferred to or from the atom to form the ion

Delocalized electron

the electrons involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom

Ionic bond

the electrostatic force that holds oppositely charged particles together

lower

the energy of an ionic compound is ___ than that of the separate elements that formed it

Ionization energy

the energy required to remove an electron from an atom in its gaseous atom; generally increases in moving from left to right across a period and increases in moving down a group

Lattice energy

the energy required to separate one mole of the ions of an ionic compound, which is directly related to the size of the ions bonded and is also affected by the charge of the ions

Lanthanide series

the f-block elements from period 6 that follow the element lanthanum

Actinide series

the f-block elements from period 7 that follow the element actinium

chemical bond

the force that holds two atoms together is called a ____

Chemical bond

the force that holds two atoms together; may form by the attraction of a positive ion for a negative ion or by sharing electrons

reactant; reactant; product arrow, + sign, g, g, g

the fuel for the space shuttle is hydrogen, which burns in oxygen to produce water vapor and energy. in this chemical reaction, hydrogen is a __, oxygen is a ___, and water vapor is a __. in this chemical equation for this reaction, a ___ is used to separate hydrogen and oxygen from water vapor and energy. a ____ is used to separate the symbols for hydrogen and oxygen. a ___ symbol is used to tell the state of hydrogen in the reaction, a ___ symbol is used for the state of oxygen, and a ___ symbol is used for the state of water vapor

-ite

the name for the ion with fewer oxygen atoms ends with ___

number of electrons

the number of bonding pairs in a molecule is not equal to the ____

hexa-

the prefix ___ indicates six atoms

four

the prefix tetra- indicates __ atoms

Chemical reaction

the process by which the atoms of one or more substances are rearranged to form different substances *changes in temperature, color, odor, and physical state

pseudo-noble gas formations

the relatively stable electron structures developed by loss of electrons in certain elements of groups 3,4,13,14 are called ____

-ide

the second element in the formula of a binary compound is named using the suffix___

Solvent

the substance that dissolves a solute to form a solution; the most plentiful substance in the solution ex) water mixed with sugar/salt

negative

to find the total number of electrons available for bonding in a ___ ion, you should add the ion charge to the total number of valence electrons of the atoms present

law of conservation of mass

total mass of the reacting substances is always equal to the total mass of products

Skeleton equation

uses chemical formulas to identify reactants and products ex) 2 Fe(s) + 3Cl₂(g) -> 2FeCl₃(s)

Word equation

uses words to indicate reactants and products of chemical reactions ex) A + B -> AB Iron (s) + chlorine (g) -> Iron III chloride (s)

- adjust the coefficients to the smallest whole-number ratio (2,3,2) - coefficient appears in front of formula in a chemical equation - chemical equations are balanced when the same number of each kind of atom appears in the reactants and the products

what are the three steps in balancing equations?

can be either positive or negative

what charge are ions

positive

what charge is a nucleus

Oxygen

what is always present in a combustion reaction?

trigonal planar

what is the molecular shape of AlCl₃

linear

what is the molecular shape of BeCl₂

tetrahedral

what is the molecular shape of CH₄

trigonal pyramidal

what is the molecular shape of PH₃

octahedral

what is the molecular shape of SF₆

exothermic

when a covalent bond occurs, bond dissociation energy is released, and the process is ___

4

when carbon and oxygen bond, the molecule contains __ pairs of bonding electrons

covalent bond

when sharing of electrons occurs, the attachment between atoms that results is called a ___

molecule

when two or more atoms bond by means of electron sharing, the resulting particle is called a ___

the shorter the bond, the stronger the bond

which of the following relationships relating to bond length is generally correct?

2

write diatomic elements with ___ as the subscript

Zn(SCN)₂

zinc thiocyanate


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