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

K12 Standards

north-carolina-k-12-science-standard-course-of-study

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

원자는 양성자와 전자의 수가 같은 중성 입자입니다. 원소는 변하지 않는 양성자의 수에 의해 정의되지만, 많은 원자들은 하나 이상의 전자를 얻거나 잃어서 전하를 띤 입자가 될 수 있습니다. 원자나 분자가 전자를 얻거나 잃으면 그것을 이온이라고 합니다.

양성자에 비해 질량이 훨씬 작은 전자는 원자 질량에 크게 영향을 주지 않습니다. 그러므로, 이온의 원자 질량은 본질적으로 중성 원자의 원자 질량과 동일합니다. 원자나 분자가 전자를 잃으면 양이온이라고 합니다.

양이온은 양전하를 가진 양성자가 음전하를 가진 전자보다 많기 때문에 양전하를 띱니다. 양이온에는 원소와 동일한 이름을 지정하고 그 뒤에 이온이라는 단어를 붙입니다. 칼슘 원자에는 20개의 양성자와 20개의 전자가 있습니다.

이 원소는 두 개의 전자를 잃으면 20개의 양성자와 18개의 전자를 가진 칼슘 이온이 됩니다. 이제 음전하보다 양전하가 두 개 더 많기 때문에, 전체적으로 양전하 2를 띱니다. 이온의 화학 기호는 오른쪽 위첨자 위치에 전하를 기록한 원자의 화학 기호로 되어 있습니다.

따라서 칼슘 이온의 화학 기호는 C-A-2+로 표기됩니다. 원자나 분자가 전자를 얻으면 음이온이라고 합니다. 음이온은 양성자보다 전자가 더 많기 때문에 음전하를 띱니다.

음이온의 영어 이름은 원소 이름에 접미사 ide를 추가하여 이름을 지정합니다. 불소 원자에는 9개의 양성자와 9개의 전자가 있습니다. 불소는 하나의 전자를 얻어 9개의 양성자와 10개의 전자를 가진 불소 이온이 됩니다.

현재 양전하보다 음전하가 한 개 더 많기 때문에 음전하 1을 띱니다. 이때 불소의 화학 기호는 F 마이너스라고 씁니다. 양전하 한 개 또는 음전하 한 개를 가진 이온의 경우 1은 일반적으로 생략됩니다.

원자들은 특정한 수의 전자를 잃거나 얻어서 이온을 형성합니다. 전형 원소에 의해 형성된 이온의 경우 많은 전하들은 주기율표를 사용하여 예측할 수 있습니다. 주기율표 왼쪽에 있는 금속들은 전자를 보통 잃게 됩니다.

1족 알칼리 금속은 모두 하나의 전자를 잃어서 양전하를 갖고 이온이 됩니다. 2족 알칼리 토금속은 두 개의 전자를 잃고 양전하 2를 띱니다. 주기율표의 오른쪽에 있는 비금속은 전자를 얻습니다.

17족 할로겐은 하나의 전자를 얻어서 음전하 1을 띱니다. 16족 원소들은 두 개의 전자를 얻어서 음전하 2를 띱니다. 많은 전이 금속은 서로 다른 전하를 가진 양이온을 형성할 수 있습니다.

18족 비활성 기체는 일반적으로 이온을 형성하지 않습니다.

<ol>
	<li>Jensen, William B. "이온 전하의 적절한 작성." 화학 교육 저널 89, no. 8 (2012) : 1084-1085.</li>
	<li>슈미트, 롤랜드. "비활성 기체 구성 - 원동력이 아니라 화학에서 게임의 규칙." 화학 교육 저널 80, no. 8 (2003) : 931.</li>
	<li>Gillespie, Ronald J. "전자 밀도, 원자 전하, 이온 결합, 공유 결합 및 극성 결합." 화학 교육 저널 78, no. 12 (2001): 1688. 
	 </li>
</ol>

이온 및 이온 전하

일반적인 화학 반응에서 각 원자의 양성자와 중성자를 포함하여 원소를 식별하는 핵은 변하지 않습니다. 그러나 전자는 다른 원자로부터의 이동에 의해 원자에 추가될 수도 있고, 다른 원자로의 이동에 의해 손실될 수도 있고, 다른 원자와 공유될 수도 있습니다. 원자 간 전자의 이동과 공유는 원소의 화학을 지배합니다. 일부 화합물이 형성되는 동안 원자는 전자를 얻거나 잃어 이온이라는 전기를 띤 입자를 형성합니다.

원자가 전자를 잃으면 양이온이라는 양이온이 형성됩니다. 양이온은 전자보다 더 많은 양성자를 가지고 있습니다. 마찬가지로 원자가 전자를 얻으면 음이온이라는 음이온이 형성됩니다. 음이온은 양성자보다 더 많은 전자를 가지고 있습니다.

주기율표는 원자가 음이온 또는 양이온을 형성할지 여부와 생성된 이온의 전하를 예측하는 데 도움이 됩니다. 주기율표에서 가장 왼쪽에서 오른쪽으로 이동하면서 주족 금속의 원자는 이전 비활성 기체의 원자와 동일한 수의 전자를 남기기에 충분한 전자를 잃습니다. 이들은 그룹 번호와 동일한 전하를 갖는 양이온을 형성합니다. 설명하자면, 알칼리 금속(1족)의 원자는 전자 1개를 잃고 1+ 전하를 갖는 양이온을 형성합니다. 알칼리 토금속(2족)은 두 개의 전자를 잃고 2+ 전하를 갖는 양이온을 형성합니다. 예를 들어, 20개의 양성자와 20개의 전자를 가진 중성 칼슘 원자는 쉽게 전자 2개를 잃습니다. 그 결과 20개의 양성자, 18개의 전자 및 2+ 전하를 갖는 양이온이 생성됩니다. 앞의 비활성 기체인 아르곤의 원자와 동일한 수의 전자를 갖고 있으며 기호는 Ca2^+입니다. 금속 이온의 이름은 그것이 형성되는 금속 원자의 이름과 동일하므로 Ca2^+를 칼슘 이온이라고 합니다.

주기율표의 맨 오른쪽에서 왼쪽으로 이동하면 비금속 원소의 원자는 일반적으로 주기율표의 다음 비활성 기체 원자와 동일한 수의 전자를 제공하기에 충분한 전자를 얻습니다. 그들은 희가스에서 왼쪽으로 이동한 그룹의 수와 동일한 음전하를 갖는 음이온을 형성합니다. 예를 들어, 17족 원소(희가스의 왼쪽 한 족)의 원자는 전자 1개를 얻고 1- 전하를 갖는 음이온을 형성합니다. 16족 원소(남은 2족)의 원자는 2개의 전자를 얻고 2− 전하를 갖는 이온을 형성합니다. 예를 들어, 35개의 양성자와 35개의 전자를 가진 중성 브롬 원자는 1개의 전자를 얻어 36개의 전자를 제공할 수 있습니다. 그 결과 양성자 35개, 전자 36개, 1-전하를 갖는 음이온이 생성됩니다. 다음 비활성 기체인 크립톤의 원자와 동일한 수의 전자를 갖고 있으며 기호는 Br^-입니다.

이온의 전하와 주기율표에서의 그룹 위치 사이의 추세는 많은 경우 지침으로 사용될 수 있습니다. 그러나 주기율표의 중심으로 갈수록 예측값은 감소합니다. 전이금속과 일부 다른 금속은 표의 위치에 따라 예측할 수 없는 가변 전하를 나타내는 경우가 많습니다. 예를 들어, 구리는 1+ 또는 2+ 전하를 갖는 이온을 형성할 수 있고, 철은 2+ 또는 3+ 전하를 갖는 이온을 형성할 수 있습니다.

이 문서는 에서 발췌되었습니다 <a href="https://openstax.org/books/chemistry-2e/pages/2-6-molecular-and-ionic-compounds">Openstax, Chemistry 2e, Section 2.6: Molecular and Ionic Compounds</a>.

일반적인 화학 반응에서 각 원자의 양성자와 중성자를 포함하고 원소를 식별하는 핵은 ...

Education

교육

JoVE Core

Chemistry

화학

하나

Atoms and Elements

원자와 원소

KEY TERMS AND CONCEPTS

주요 용어 및 개념

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

chemistry

JoVE Core 화학은 간결하고 이해하기 쉬운 애니메이션을 통해 일반 화학 개념을 설명합니다. 또한, 과학자가 직접 고전실험과 연구실험을 진행하는 실사 영상을 제공합니다.

Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-1

motion-and-stability-forces-and-interactions

Motion And Stability: Forces And Interactions

HS-PS2-6

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Atoms

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.13

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.a

PS.4

PS.4.a

Arizona Science Standards

HS+C.P1

HS+C.P1U1.1

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

9-12.PS.3.4.d

Florida Department of Education

SC.912.P.8

SC.912.P.8.4

Texas Essential Knowledge and Skills

Chemistry and Physics

IPC.7

IPC.7.A

Georgia Standards of Excellence

SPS1.

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

There is no one solvent that can dissolve every type of solute. Some substances that readily dissolve in a certain solvent might be insoluble in a ...

Colloids

Children at play often make suspensions such as mixtures of mud and water, flour and water, or a suspension of solid pigments in water known as tempera ...

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 ...

phase-transitions-vaporization-and-condensation

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

physical-and-chemical-properties-of-matter

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 ...

molecular-comparison-of-gases-liquids-and-solids

Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

comparing-intermolecular-forces-melting-point-boiling-point

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 ...

atomic-radii-and-effective-nuclear-charge

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

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

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

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

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 ...

structure-and-nomenclature-of-alcohols-and-phenols

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

Description

Transcript

More videos by Standards