Name: predicting ion charges on the periodic table
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 3 min 27 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.1.5

Ions and Ionic Charges

Atomy to neutralne cząstki o równej liczbie protonów i elektronów. Pierwiastek jest zdefiniowany przez liczbę protonów, która się nie zmienia; Jednak wiele atomów może zyskać lub stracić jeden lub więcej elektronów, aby stać się naładowaną cząstką.

Kiedy atom lub cząsteczka zyskuje lub traci elektrony, nazywa się to jonem. Elektrony, mając znacznie mniejszą masę niż protony, nie przyczyniają się znacząco do masy atomowej. Dlatego masa atomowa jonu jest zasadniczo taka sama jak masa atomowa atomu neutralnego.

Kiedy atomy lub cząsteczki tracą elektrony, nazywa się je kationami. Kationy mają ładunek dodatni, ponieważ mają więcej protonów, które mają ładunek dodatni, niż elektronów, które mają ładunek ujemny. Kationy otrzymują taką samą nazwę jak ich pierwiastek, po którym następuje słowo jon.

Atom wapnia ma 20 protonów i 20 elektronów. Traci dwa elektrony, aby stać się jonem  wapnia z 20 protonami i 18 elektronami.  Ponieważ ma teraz dwa ładunki dodatnie więcej niż ujemne, ma ogólny ładunek dodatni dwa. 

Symbol chemiczny jonu jest zapisywany jako symbol chemiczny atomu z ładunkiem zapisanym w prawej pozycji indeksu górnego. Symbol chemiczny jonu wapnia jest zatem zapisywany jako Ca2+.

Kiedy atomy lub cząsteczki zyskują elektrony, nazywa się je anionami. Aniony mają ładunek ujemny, ponieważ mają więcej elektronów niż protonów. Nazwy anionów są dodawane przez dodanie sufiksu "-ide" do nazwy ich elementu.

Atom fluoru ma 9 protonów i 9 elektronów. Fluor zyskuje jeden elektron, stając się jonem fluorkowym z 9 protonami i 10 elektronami. Ponieważ ma teraz o jeden ładunek ujemny więcej niż ładunek dodatni, ma ogólny ładunek ujemny.

Symbol chemiczny fluoru jest zapisywany jako F−.  Ten jest zwykle pomijany dla jonów o dodatnim lub ujemnym ładunku.

Atomy tracą lub zyskują określoną liczbę elektronów podczas tworzenia jonu. Wiele ładunków jonów utworzonych przez główne pierwiastki grupy można przewidzieć za pomocą układu okresowego pierwiastków. 

Metale po lewej stronie układu okresowego stracą elektrony. Wszystkie metale alkaliczne grupy 1 tracą jeden elektron i mają dodatni jeden ładunek, gdy stają się jonem. Metale ziem alkalicznych z grupy 2 tracą dwa elektrony i mają dodatni ładunek dwu. 

Niemetale, po prawej stronie układu okresowego pierwiastków, zyskają elektrony. Halogeny z grupy 17 zyskują jeden elektron i mają ładunek ujemny. Grupy 16 pierwiastków zyskują dwa elektrony i będą miały ujemny ładunek dwu.

Wiele metali przejściowych może tworzyć kationy o różnych ładunkach. Gazy szlachetne z grupy 18 na ogół nie tworzą jonów.

<ol>
	<li>Jensen, William B. "Prawidłowy zapis ładunków jonowych." Journal of Chemical Education 89, nr 8 (2012): 1084-1085.</li>
	<li>Schmid, Roland. "Konfiguracja gazów szlachetnych – nie siła napędowa, ale reguła gry w chemii." Dziennik Edukacji Chemicznej 80, nr 8 (2003): 931.</li>
	<li>Gillespie, Ronald J. "Gęstości elektronów, ładunki atomowe oraz wiązania jonowe, kowalencyjne i polarne." Journal of Chemical Education 78, nr 12 (2001): 1688. 
	 </li>
</ol>

jony i ładunki jonowe

W zwykłych reakcjach chemicznych jądro — które zawiera protony i neutrony każdego atomu, i w ten sposób identyfikuje pierwiastek — pozostaje niezmienione. Elektrony można jednak dodawać do atomów poprzez przeniesienie z innych atomów, utracić poprzez przeniesienie do innych atomów lub współdzielić z innymi atomami. Przenoszenie i dzielenie elektronów między atomami reguluje chemię pierwiastków. Podczas tworzenia niektórych związków atomy zyskują lub tracą elektrony, tworząc elektrycznie naładowane cząstki zwane jonami.

Kiedy atom traci elektrony, tworzy jon dodatni zwany kationem. Kationy mają więcej protonów niż elektronów. Podobnie, gdy atom zyskuje elektrony, tworzy jon ujemny zwany anionem. Aniony mają więcej elektronów niż protonów.

Układ okresowy pomaga przewidzieć, czy atom utworzy anion, czy kation, a także jaki będzie ładunek powstałego jonu. Poruszając się od skrajnej lewej do prawej strony układu okresowego, atomy metali z grupy głównej tracą wystarczającą ilość elektronów, aby pozostawić je z taką samą liczbą elektronów, jak atom poprzedzającego gazu szlachetnego. Tworzą one kationy o ładunku równym liczbie grupowej. Aby to zilustrować, atom metalu alkalicznego (grupa 1) traci jeden elektron i tworzy kation o ładunku 1+; metal ziem alkalicznych (grupa 2) traci dwa elektrony i tworzy kation o ładunku 2+, i tak dalej. Na przykład obojętny atom wapnia zawierający 20 protonów i 20 elektronów łatwo traci dwa elektrony. Daje to kation z 20 protonami, 18 elektronami i ładunkiem 2+. Ma taką samą liczbę elektronów jak atomy poprzedniego gazu szlachetnego, argonu, i jest symbolizowany jako Ca2+. Nazwa jonu metalu jest taka sama jak nazwa atomu metalu, z którego się składa, dlatego Ca2+ nazywany jest jonem wapnia.

Poruszając się od skrajnej prawej do lewej strony układu okresowego, atomy pierwiastków niemetalicznych zazwyczaj zyskują wystarczającą liczbę elektronów, aby zapewnić im tę samą liczbę elektronów, co atom następnego gazu szlachetnego w układzie okresowym. Tworzą aniony o ładunku ujemnym równym liczbie grup przesuniętych w lewo od gazów szlachetnych. Na przykład atomy pierwiastków z grupy 17 (jedna grupa na lewo od gazów szlachetnych) zyskują jeden elektron i tworzą aniony o ładunku 1-; atomy pierwiastków z grupy 16 (pozostały dwie grupy) zyskują dwa elektrony i tworzą jony o ładunku 2-, i tak dalej. Na przykład obojętny atom bromu, mający 35 protonów i 35 elektronów, może zyskać jeden elektron, aby aby łącznie otrzymać 36 elektronów. Daje to anion z 35 protonami, 36 elektronami i ładunkiem 1-. Ma on taką samą liczbę elektronów, jak atomy następnego gazu szlachetnego, kryptonu, i jest symbolizowany jako Br−.

Trend między ładunkiem jonu, a pozycją grupy w układzie okresowym może w wielu przypadkach służyć jako wskazówka. Jednak jego wartość predykcyjna maleje w miarę przesuwania się w stronę środka układu okresowego. Metale przejściowe i niektóre inne metale często wykazują zmienne ładunki, których nie można przewidzieć na podstawie ich położenia w tabeli. Na przykład, miedź może tworzyć jony o ładunku 1+ lub 2+, a żelazo może tworzyć jony o ładunku 2+ lub 3+.

Jony i ładunki jonowe

W zwykłych reakcjach chemicznych jądro - które zawiera protony i neutrony każdego atomu, a tym samym identyfikuje pierwiastek - pozostaje ...

Education

JoVE Core

Chemistry

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Atoms and Elements

Atomy i pierwiastki

KEY TERMS AND CONCEPTS

Kluczowe terminy i pojęcia

predicting ion charges on the periodic table

Ion charges can often be predicted from an element’s position on the periodic table. In chemical reactions, the nucleus stays unchanged, but electrons may be transferred, lost, or shared. When atoms gain or lose electrons during compound formation, they become ions, which are electrically charged particles.

A positive ion is called a cation. A cation has more protons than electrons because it lost electrons. A negative ion is called an anion. An anion has more electrons than protons because it gained electrons.

The periodic table gives useful clues about ion charge. Main-group metals on the far left usually lose electrons until they have the same number of electrons as the preceding noble gas. Their cation charge often matches the group number. For example, a Group 1 alkali metal forms a 1+ cation, and a Group 2 alkaline earth metal forms a 2+ cation.

Calcium shows this pattern clearly. A neutral calcium atom has 20 protons and 20 electrons. It can lose two electrons to form Ca2+, which has 20 protons, 18 electrons, and a 2+ charge. This ion has the same number of electrons as argon. The name of the metal ion is the same as the metal atom, so Ca2+ is called a calcium ion.

Nonmetals on the far right usually gain electrons to reach the electron count of the next noble gas. Their anion charge often matches how many groups they are away from the noble gases. Group 17 elements usually gain one electron to form 1− anions, and Group 16 elements usually gain two electrons to form 2− anions.

Bromine is one example. A neutral bromine atom has 35 protons and 35 electrons. It can gain one electron to form Br− with 35 protons, 36 electrons, and a 1− charge. This ion has the same number of electrons as krypton. The trend between group position and ion charge helps in many cases, but it becomes less reliable near the center of the periodic table. Transition metals and some other metals often have variable charges. Copper can form 1+ or 2+ ions, and iron can form 2+ or 3+ ions.

Predicting Ion Charges on the Periodic Table

predicting-ion-charges-on-the-periodic-table

the atomic theory of matter

Dalton’s Laws and Early Atomic Ideas

Dalton’s atomic theory explains matter with atoms, elements, and compounds. It also shows how chemical changes follow simple laws. This idea gave chemistry a microscopic model for what can be seen in the lab. The earliest recorded ideas about matter came from ancient Greek philosophers. Leucippus and Democritus said all matter was made of tiny, finite particles called atomos, meaning “indivisible.” Aristotle and others later argued that matter was made from four elements: fire, earth, air, and...

subatomic particles

Atomic Structure: Protons, Neutrons, and Electrons

Atomic structure is built from three subatomic particles: protons, neutrons, and electrons. Atoms make up all matter, and these particles explain an atom’s mass and charge. The electron was first identified at the end of the 19th century by J.J. Thomson. He used a cathode ray tube, a sealed glass tube with almost all the air removed and two metal electrodes. When high voltage was applied, a visible beam called a cathode ray formed. The beam bent toward positive charge and away from negative...

elements: chemical symbols and isotopes

Reading Element Symbols and Isotope Notation

Chemical symbols and isotope notation help identify elements and their atoms. A chemical symbol is an abbreviation for an element or a single atom of that element. Mercury, for example, is written as Hg. The same symbol can point to one atom in the microscopic domain or to many atoms of the element in a container or sample. Many symbols come from the element’s common English name. Others come from Latin, Greek, or German names. Aluminum uses Al, while iron uses Fe from the Latin word Ferrum.

ions and ionic charges

Ion charges can often be predicted from an element’s position on the periodic table. In chemical reactions, the nucleus stays unchanged, but electrons may be transferred, lost, or shared. When atoms gain or lose electrons during compound formation, they become ions, which are electrically charged particles. A positive ion is called a cation. A cation has more protons than electrons because it lost electrons. A negative ion is called an anion. An anion has more electrons than protons because it...

the periodic table

Periodic Table Patterns and Element Groups

The periodic table organizes elements by repeating patterns in their properties. Chemists first noticed that some elements behaved alike, so they grouped them by chemical behavior. Lithium, sodium, and potassium are one example. They are shiny and conduct heat and electricity well. Calcium, strontium, and barium form another group with similar physical and chemical properties. Yet these two groups are not the same. The lithium group is much more reactive, and its elements form oxygen compounds...

atomic mass

Average Atomic Mass and Isotopes

Average atomic mass explains why many elements on the periodic table have decimal values. Atoms are extremely small, so scientists use the atomic mass unit, or amu, to measure them. A carbon atom weighs less than 2 × 10−23 g, and the amu is defined from carbon-12. One amu is exactly 1/12 the mass of one carbon-12 atom, which is 1.6605 × 10−24 g. The dalton (Da) and the unified atomic mass unit (u) mean the same thing as the amu. For a single atom, atomic mass is usually close to its mass...

molar mass

Mole, Mass, and Avogadro’s Number

The mole links mass and the number of particles in a substance. It gives chemists a standard way to count atoms and molecules in samples that are far too small to see. It also helps show why substances with the same kinds of atoms can still have very different properties, like water, H2O, and hydrogen peroxide, H2O2. The mole is an amount unit, like a pair or a dozen. One mole contains 6.02214076 × 10^23 discrete entities, such as atoms or molecules. This number is usually rounded to 6.022 ×...

key terms and concepts

Learn how the periodic table helps predict cation and anion charges, with examples like calcium, bromine, copper, and iron for grades 9–12.

Predicting Ion Charges on the Periodic Table | JoVE K12

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Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-1

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Motion And Stability: Forces And Interactions

HS-PS2-6

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Study Of Matter

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Tennessee Academic Standards

Matter and Its Interactions

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CH.2

CH.2.a

PS.4

PS.4.a

Arizona Science Standards

HS+C.P1

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HS.P1

HS.P1U1.2

Alabama Course of Study Science

9-12.C.1.1.a

9-12.C.1.1.b

9-12.PS.3.4

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Florida Department of Education

SC.912.P.8

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Texas Essential Knowledge and Skills

Chemistry and Physics

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Properties of Atoms, Ions, and Isotopes

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

Elements: Chemical Symbols and Isotopes

A chemical symbol is an abbreviation used to indicate an element or an atom of an element. For example, the symbol for mercury is Hg. The same symbol is ...

Molecules and Compounds

Atoms and Molecules

Everything in the universe is made up of matter, and matter is composed of a combination of elements. An atom is the smallest unit of ...

Solution Formation

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Colloids

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Construct an explanation to classify matter as a pure substance or mixture; homogeneous or heterogeneous; element or compound; solution, colloid or suspension.

PS.PSc.1.1

Phase Transitions

Whether solid, liquid, or gas, a substance&#39;s state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the ...

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Phase Transitions: Vaporization and Condensation

The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize ...

Vapor Pressure

When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally ...

Clausius-Clapeyron Equation

The equilibrium between a liquid and its vapor depends on the temperature of the system; a rise in temperature causes a corresponding rise in the vapor ...

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy ...

phase-transitions-sublimation-and-deposition

Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and ...

Heating and Cooling Curves

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. ...

Use models to compare the phases of matter and the physical changes they undergo.

PS.PSc.1.2

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Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

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Molecular Comparison of Gases, Liquids, and Solids

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Intermolecular vs Intramolecular Forces

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Intermolecular Forces

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

Carry out investigations to compare physical and chemical properties of matter.

PS.PSc.1.3

The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

The Bohr Model

Following the work of Ernest Rutherford and his colleagues in the early twentieth century, the picture of atoms consisting of tiny dense nuclei surrounded ...

Emission Spectra

When solids, liquids, or condensed gases are heated sufficiently, they radiate some of the excess energy as light. Photons produced in this manner have a ...

The de Broglie Wavelength

In the macroscopic world, objects that are large enough to be seen by the naked eye follow the rules of classical physics. A billiard ball moving on a ...

The Uncertainty Principle

Werner Heisenberg considered the limits of how accurately one can measure properties of an electron or other microscopic particles. He determined that ...

Use models to interpret the data presented in Bohr diagrams and electron dot diagrams for neutral atoms of elements 1 through 18.

PS.PSc.1.4

In ordinary chemical reactions, the nucleus &mdash; which contains the protons and neutrons of each atom and thus identifies the element &mdash; remains ...

Use models to compare representations of atoms, ions, and isotopes.

The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

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Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

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Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Halogens

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Noble Gases


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

Use the Periodic Table as a model to predict the relative properties (metallic/nonmetallic character, ionic charge, and reactivity) and arrangement of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.PSc.1.6

Types of Chemical Bonds

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Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

Construct an explanation to classify the type of chemical bond that occurs (covalent, ionic, or metallic) in a given substance.

PS.PSc.2.1

Nomenclature of Alkanes

In the late 19th-century, the number of new chemical compounds discovered increased tremendously. Hence, the necessity arose to develop a naming system ...

Nomenclature of Alkenes

The IUPAC naming system for alkenes replaces -an- with -en- in the corresponding parent alkanes. Accordingly, a simple alkene replaces the -ane suffix of ...

Nomenclature of Alkynes

Alkynes are unsaturated hydrocarbons characterized by the presence of carbon-carbon triple bonds and have a general formula CnH2n-2. The nomenclature of ...

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Structure and Nomenclature of Alcohols and Phenols

Overview 
Alcohols are one of the most important functional groups in organic chemistry. The name of alcohol comes from the hydrocarbon from which it is ...

Structure and Nomenclature of Ethers

Structure and Bonding
Ethers are organic compounds with an ether functional group which is characterized by an oxygen atom connected to two &#8212; ...

IUPAC Nomenclature of Aldehydes

Aldehydes are named based on the systematic nomenclature rules set by the IUPAC. For acyclic aldehydes, the longest carbon chain containing the aldehydic ...

Use models to apply International Union of Pure and Applied Chemistry (IUPAC) conventions to name and write formulas for simple compounds.

PS.PSc.2.2

Understand types, properties, and structure of matter.

Predicting Ion Charges on the Periodic Table

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