Name: how acids and bases form ions
Uploaded: 2020-09-03T13:38:26.000Z
Duration: 3 min 26 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.2.4

Acids, Bases and Neutralization Reactions

人間の胃は 食物の消化を助ける塩酸を含む 胃液を含んだ筋肉の器官です ある種の食品は 私達の胃の酸性度を上げ 酸の逆流を引き起こします アルカリ性の食品や 制酸剤のような 塩基性のものを摂取すると 余分な酸が中和され ヒリヒリとした感覚が和らぎます これが酸と塩基の反応の一例です 最も単純な酸は 解離可能な 水素原子を含む物質です 水溶液中では 正に帯電した水素イオンである プロトンと それに対応する 陰イオンが放出されます プロトンは水分子と反応して ヒドロニウムイオンを 形成します 例えば 硝酸の水溶液には ヒドロニウムイオンと 硝酸イオンが含まれています 他の一般的に知られている酸は 塩酸 硫酸 リン酸です 酸は 分子あたりの 解離性水素原子の数に応じて モノプロトン性または ポリプロトン性を示します 解離性水素が1個ずつの 塩酸と硝酸はモノプロトン性の 酸の例であり 硫酸とリン酸は ポリプロトン性の酸です 硫酸は二プロトン性で 2つのプロトンを 順次放出しますが リン酸は三プロトン性で プロトンを3段階で順次放出します 最も単純な塩基は 水溶液中で負に帯電した 水酸化物イオンを 生成する化合物です 簡単に識別できる塩基は 水酸化ナトリウム 水酸化カリウム 水酸化カルシウムなどの 水酸基を含んでいます このような塩基は 水に添加されると 水酸化物イオンと対応する 金属陽イオンに解離します アンモニアのような 非水酸化物塩基は 水分子からプロトンを受け入れて 水と反応し アンモニウムイオンと 水酸化物イオンを生成する 一般に 酸と塩基は反応して 水と塩を生成します 酸と塩基の反応は 酸から供給される プロトンのモル数と塩基から 供給される水酸化物イオンの モル数が等しい場合は 中和反応とも呼ばれています 例えば 硝酸水溶液と 水酸化カリウム水溶液を 等量混合すると 溶液に供給される ヒドロニウムイオンと 水酸化物イオンの 量も等しくなります ヒドロニウムイオンと 水酸化物イオンは 結合して水を形成することで 完全に中和され ヒドロニウムイオンや 水酸化物イオンは残りません さらに 硝酸アニオンと カリウム陽イオンが対になって 硝酸カリウムという 塩を形成します 中和反応の中にはガス発生反応 と呼ばれるものがあります 例えば 塩酸と亜硫酸カリウムが 反応して 亜硫酸-亜硫酸塩平衡系を介して 塩化カリウム 水 二酸化硫黄ガスを 生成します

酸、塩基、中和反応

酸塩基反応とは、水素イオン（ H+ ）がある化学種から別の化学種に移動する反応です。 このような反応は、細胞や湖、海洋内の化学的変化から、産業規模での肥料、医薬品、その他社会に不可欠な物質の生産まで、数多くの自然・技術的なプロセスにとって重要なものとなっています。 
 
 酸を定義する方法はいくつかあります。 水溶液の場合、酸は溶解して水素イオンを生成する物質のことです。 
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-01.png" style="height: 40px;" />
 
 これは、スウェーデンの化学者である スヴァンテ・アレニウス (1859 – 1927) にちなんで名付けられた酸の定義です。 H+記号で表される水素イオンはプロトンと呼ばれます。 溶液中では、プロトンは、酸素の単独ペアを通じて水分子と化学的に結合し、ヒドロニウムイオン、 H3O+ を形成します。 
 
 <img alt="Eq2" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-02.png" style="height: 40px;" />
 
 酸のイオン化の化学方程式は、次のように書かれます。 
 
 <img alt="Eq3" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-03.png" style="height: 40px;" />
 
 この方法で水と完全に反応する酸を強酸と呼びます。 HCl 、 HNO3 、および HBr は、その例です。 
 
 日常生活で遭遇するほとんどの酸は弱酸です。 果物中のクエン酸、酢中の酢酸、牛乳中の乳酸などがその例です。 弱酸のよく知られた例は酢酸、食用酢の主要な原料です。 一般的な条件下で水に溶解した場合、イオン化した状態CH3CO2−では酢酸分子の約 1% しか存在しません。 
 
 <img alt="Eq4" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-04.png" style="height: 40px;" />
 
 上の方程式で二重矢印を使用することは、このプロセスの部分的な反応であることを表しています。 
 
 塩基は、水酸化物イオンを生成するために水に溶解する物質です。 最も一般的な塩基は、アルカリまたはアルカリ土類の金属陽イオン（ 1 および 2 族）と水酸化物イオン（ 例えばNaOH 、 Ca(OH)2など）で構成されるイオン化合物です。 前述した酸化合物とは異なり、これらの化合物は水と化学的に反応しません。その代わり、溶液に水酸化物イオンを直接放出して溶解および解離します。 たとえば、 KOH とBa(OH)2 は水に溶解して完全に解離し、陽イオン（それぞれ K+ と Ba2+ ）と水酸化物イオン（ OH−）を生成します。 これらの塩基は、水中で完全に解離する他の水酸化物と同様、強い塩基と考えられています。 
 
 水中の水酸化ナトリウムの溶解を例として考えてみます。 
 
 <img alt="Eq5" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-05.png" style="height: 40px;" />
 
 この方程式は水酸化ナトリウムが塩基であることを示しています。 水に溶解すると、 NaOH は解離して Na+ および OH−イオンを生成します。 これは水酸化物イオンを含む他のイオン化合物にも当てはまります。 一般的な条件下でイオン化合物が水に溶解した時点で解離プロセスが基本的に完了するため、 NaOH やその他のイオン水酸化物はすべて強力な塩基として分類されます。 
 
 イオン水酸化物とは異なり、一部の化合物は、水分子と化学的に反応することで、水酸化物イオンを生成します。 いずれの場合も、これらの化合物は部分的にしか反応しないため、弱い塩基として分類されます。 この種の化合物は自然にも豊富にあり、さまざまな技術において重要な商品となっています。 たとえば、弱塩基のアンモニアの世界生産量は、農業用肥料、他の化合物の化学合成用原料、家庭用洗剤の有効成分として広く使用されているため、年間 100 トンを超えます。 水に溶解した場合、アンモニアは水酸化物イオンに部分的に反応します（以下を参照）。 
 
 <img alt="Eq6" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-06.png" style="height: 40px;" />
 
 これは、定義上、水分子からアンモニア分子への H+ イオンの移動を伴う酸塩基反応です。 一般的な条件下では、 NH4+ イオンとして存在するのは溶存アンモニアの約 1% のみです。 
 
 中和反応とは、反応物質が酸および塩基（かつ水ではない）であり、生成物が塩および水であることが多い特定のタイプの酸塩基反応です。  
 
 <img alt="Eq7" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-07.png" style="height: 40px;" />
 
 中和反応を説明するために、胃酸過多（ HCl ）による症状を緩和するために、代表的な制酸剤であるマグネシアミルク（固体のMg(OH)2の水性懸濁液）を摂取した場合にどうなるかを検討してみます。 
 
 <img alt="Eq8" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-08.png" style="height: 40px;" />
 
 水に加えて、この反応は塩である塩化マグネシウムを生成することに注意してください。 （強または弱）酸からの H+ （aq）は、塩基からの（または水と弱塩基の反応によって生成された） OH−（ aq）と結合して H2O (l)を形成します。 例えば、 HCl （強酸）と NaOH （強塩基）の水溶液間の反応は次のように記述されます。 
 
 <img alt="Eq9" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-09.png" style="height: 40px;" />
 
 HCl と NaOH の両方で 100% イオン化が行われます。 したがって、完全なイオン方程式は次のように記述されます。 
 
 <img alt="Eq10" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-10.png" style="height: 40px;" />
 
 Cl-および Na+ はキャンセルされる傍観イオンと呼ばれ、正味のイオン方程式は次のようになります。  
 
 <img alt="Eq11" src="https://www.jovecore.com/CDNSource/lessons/1029/1029_Equations-11.png" style="height: 40px;" />
 
 このテキストは <a href="https://openstax.org/books/chemistry-2e/pages/4-2-classifying-chemical-reactions">、 OpenStax Chemistry 2e のセクション 4.2: 化学反応の分類、に基づいています。</a>

酸塩基反応とは、水素イオンH+が1つの化学種から別の化学種に移動する反応です。このような反応は、...

Education

Book

Chemistry

化学

Chemical Quantities and Aqueous Reactions

化学量と水溶液反応

chemical-quantities-and-aqueous-reactions

how acids and bases form ions

Acids and bases form ions in water through acid-base reactions. These reactions move a hydrogen ion, H+, from one chemical species to another. They matter in many natural and technological processes, from chemistry inside cells and in lakes and oceans to the large-scale production of fertilizers, pharmaceuticals, and other useful substances.

In water, an acid is a substance that produces hydrogen ions. This is the Arrhenius definition of an acid. The H+ ion is also called a proton. In solution, these protons combine with water molecules to form hydronium ions, H3O+.

Acids that react completely with water are called strong acids. Common examples include HCl, HNO3, and HBr. Most acids people encounter in daily life are weak acids. Citric acid in fruits, acetic acid in vinegar, and lactic acid in milk are examples. Acetic acid is a familiar weak acid, and under typical conditions only about 1% of its molecules are in the ionized form, CH3CO2−. A double arrow shows that this reaction is only partial.

A base is a substance that dissolves in water to yield hydroxide ions, OH−. The most common bases are ionic compounds made of alkali or alkaline earth metal cations from groups 1 and 2 with hydroxide ions, such as NaOH and Ca(OH)2. These compounds do not react chemically with water. Instead, they dissolve and dissociate, releasing hydroxide ions directly into solution.

KOH and Ba(OH)2 are examples of strong bases because they dissociate completely in water. The same is true for sodium hydroxide. When NaOH dissolves, it gives Na+ and OH− ions. Any ionic compound that contains hydroxide ions behaves this way under typical conditions, so these hydroxides are classified as strong bases.

Some compounds make hydroxide ions by reacting with water molecules instead of simply dissociating. These compounds react only partially, so they are weak bases. Ammonia is a common example. It is produced on a very large scale because it is used as an agricultural fertilizer, a starting material for chemical synthesis, and an ingredient in household cleaners. When ammonia dissolves in water, it reacts partially to form OH− and NH4+ ions. This is an acid-base reaction because H+ ions move from water molecules to ammonia molecules. Under typical conditions, only about 1% of dissolved ammonia is present as NH4+.

A neutralization reaction is a special acid-base reaction in which an acid and a base react, but water is not a reactant. The products are often a salt and water. Milk of magnesia is a common antacid made of solid Mg(OH)2 in water. It helps relieve excess stomach acid, HCl, by neutralizing it. This reaction forms water and the salt magnesium chloride.

In neutralization, H+(aq) from the acid combines with OH−(aq) from the base to make H2O(l). For example, HCl and NaOH are both completely ionized in water. Their complete ionic equation includes Na+ and Cl− ions, but these are spectator ions because they cancel out. The net ionic equation shows the essential change: H+(aq) + OH−(aq) → H2O(l).

How Acids and Bases Form Ions

precipitation reactions

Predicting Precipitation in Aqueous Reactions

Precipitation reactions happen when two aqueous solutions of soluble salts are mixed and an insoluble ionic compound forms. That solid is called a precipitate. The ions in solution exchange partners, so these reactions are also called double displacement, double replacement, exchange, or metathesis reactions. These reactions are useful in chemistry for identifying metal ions in a compound. They also support gravimetric methods, which measure composition by the mass of a substance. Whether a...

reaction stoichiometry

Using Balanced Equations to Predict Amounts

Balanced chemical equations show how much of each substance reacts and forms in a chemical change. The formulas identify the reactants and products, which helps classify the reaction. The coefficients show the relative numbers of each substance, which lets chemists measure the relationships between amounts consumed and produced. These quantitative relationships are called stoichiometry. The word comes from the Greek words stoicheion, meaning element, and metron, meaning measure. Stoichiometry...

acids, bases and neutralization reactions

Acids and bases form ions in water through acid-base reactions. These reactions move a hydrogen ion, H+, from one chemical species to another. They matter in many natural and technological processes, from chemistry inside cells and in lakes and oceans to the large-scale production of fertilizers, pharmaceuticals, and other useful substances. In water, an acid is a substance that produces hydrogen ions. This is the Arrhenius definition of an acid. The H+ ion is also called a proton. In...

limiting reactant

Limiting Reactant in Water Formation

Limiting reactants control how much product forms in a chemical reaction. In a balanced equation, the listed amounts of reactants and products are called stoichiometric amounts. In real reactions, the reactants are not always present in those exact proportions. The limiting reactant is the reactant that gets used up first. Once it is gone, the reaction stops making more product. The other reactant is called the excess reactant. Chemists often use extra amounts of one reactant to make sure the...

reaction yield

Calculating Percent Yield in Reactions

Percent yield shows how much product a chemical reaction actually makes compared with how much it should make. The expected amount is called the theoretical yield. It comes from the balanced chemical equation and the stoichiometry, or mole ratios, in that equation. The theoretical yield assumes that the limiting reactant is completely converted into the desired product. The product collected after a reaction is the actual yield. In many cases, the actual yield is lower than the theoretical...

general properties of solutions

Solvents, Solutes, and Solution Types

Solutions are common mixtures found in everyday life. Ocean water, air, and gasoline are all examples of solutions. These mixtures contain two or more types of atoms or molecules in varying amounts. A solution is a homogeneous mixture, which means its composition is uniform throughout. This is different from a heterogeneous mixture, which has a non-uniform composition. In a homogeneous mixture, the components are evenly spread out and thoroughly mixed. Every solution has a solvent and a...

solution concentration and dilution

Molarity and Dilution in Solutions

Molarity and dilution are key ideas for describing solution concentration. Concentration means the relative amount of one component in a solution. In many solutions, one component is present in much larger amount. That component is the solvent, which acts as the medium that holds the other parts dissolved or dispersed. Water is a very common solvent, so aqueous solutions are common on Earth. A solute is the component present at a much lower concentration than the solvent. Chemists often...

electrolyte and nonelectrolyte solutions

Conductivity in Electrolyte Solutions

Electrolyte solutions conduct electricity because they contain mobile ions. The amount of current depends on how many ions are present in the aqueous solution. A solution with more dissolved ions conducts better, while a solution with few or no ions conducts poorly. Strong electrolytes dissociate completely in water. This complete dissociation is shown with a single forward arrow. Water-soluble ionic compounds such as sodium chloride split into sodium cations and chloride anions in solution.

solubility of ionic compounds

Solubility Rules for Ionic Salts

Solubility rules help predict whether ionic salts will dissolve in water. Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a set temperature and pressure. It is often measured in molarity, or moles per liter (mol/L). A compound is soluble if it dissolves in water. When a soluble salt dissolves, its ions separate and spread evenly through the solution. This physical change is called dissociation. Potassium chloride, KCl, is a simple example. Water...

chemical reactions in aqueous solutions

Aqueous Reactions and Ionic Equations

Aqueous reactions are chemical reactions that take place in water. Water is a good solvent, so it can dissolve many substances. Because of that, many chemical reactions happen in aqueous solution. In high school chemistry, these reactions are often grouped into three common patterns: precipitation, acid-base, and oxidation-reduction. A precipitation reaction happens when ions in two aqueous ionic compounds exchange partners and form an insoluble salt, called a precipitate. In an acid-base...

oxidation–reduction reactions

Redox Reactions and Oxidation Numbers

Redox reactions are chemical changes in which electrons move between reactants, and oxidation numbers help track that change. The term oxidation once referred only to reactions with molecular oxygen, but it now covers a wider reaction class called oxidation-reduction, or redox, reactions. Some redox reactions form ionic products. A simple example is the reaction between sodium and chlorine that produces sodium chloride. To follow what happens to each reactant, chemists often write...

oxidation numbers

Assigning Oxidation States in Redox Reactions

Oxidation states help track electron transfer in redox reactions. An oxidation number, also called an oxidation state, is a hypothetical number that shows the effective charge of an atom or element. Chemists assign it by using a set of rules. In an ionic compound, oxidation numbers are based on how many electrons move between reacting species. For example, when calcium chloride forms, calcium loses two valence electrons and the two chlorine atoms each gain one electron. In CaCl2, calcium has...

acids, bases, and neutralization reactions

synthesis and decomposition reactions

Building and Breaking in Chemical Reactions

Synthesis and decomposition are two redox reactions that show how substances can be built up or broken down. Synthesis means to make something, while decomposition means to break something apart. These reactions also involve chemical changes and energy changes. Synthesis reactions are also called combination reactions. In a synthesis reaction, two or more substances join to form one more complex substance. They are often written as A + B → AB or A + B → C. One example is the formation of...

scientists in action

活動する科学者たち

key terms

主要用語

key relationships & equations

主要な関係性と方程式

chapter exercises

章末問題

appendices

付録

chemical quantities and aqueous reactions

Learn how acids and bases form ions in water, including strong and weak acids, strong and weak bases, ammonia, and neutralization reactions.

How Acids and Bases Form Ions | JoVE K12

chemistry

最初の本

PS.PSc.2.6

Texas Essential Knowledge and Skills

High School

Chemistry and Physics

IPC.8

IPC.8.A

Pennsylvania State Academic Standards

Chemical Reactions

3.2.9-12.C

3.2.9-12.G

Louisiana Student Standards for Science

Matter And Its Interactions

HS-PS1-2

HS-PS1-7

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.4

Arizona Science Standards

HS+C.P1

HS+C.P1U1.5

CHEM.9

CHEM.9.B

Alabama Course of Study Science

9-12.PS.3.5.d

9-12.PS.3.6.d

Florida Department of Education

SC.912.P.8

SC.912.P.8.8

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-4.

HS-PS1-12.

Georgia Standards of Excellence

SC6.

Neutralization Reactions

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

Ions and Ionic Charges

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.

PS.PSc.1.5

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

Understand types, properties, and structure of matter.

How Acids and Bases Form Ions

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