Valence in a sentence

(1) The valence number of neon is 0.

(2) The valence number of sodium is 1.

(3) The valence number of silver is 1.

(4) The valence number of helium is 0.

(5) Oxygen has a valence number of -2.

(6) Sodium has a valence number of +1.

(7) Carbon has a valence number of +4.

(8) Sulfur has a valence number of -2.

(9) The valence number of calcium is 2.

(10) The valence number of sodium is +1.

Valence sentence

(11) The valence number of carbon is +4.

(12) Calcium has a valence number of +2.

(13) The valence number of hydrogen is 1.

(14) The valence number of fluorine is 1.

(15) The valence of zinc is typically 2+.

(16) Chlorine has a valence number of -1.

(17) The valence number of calcium is +2.

(18) Fluorine has a valence number of -1.

(19) Nitrogen has a valence number of -3.

(20) The valence number of magnesium is 2.

Valence make sentence

(21) The valence number of hydrogen is +1.

(22) The valence of oxygen is typically 2-.

(23) The valence of sodium is typically 1+.

(24) The valence of sulfur is typically 2-.

(25) The valence of iodine is typically 1-.

(26) The valence of silver is typically 1+.

(27) The valence number of magnesium is +2.

(28) The valence number of potassium is +1.

(29) Phosphorus has a valence number of -3.

(30) The valence of calcium is typically 2+.

Sentence of valence

(31) The valence of bromine is typically 1-.

(32) The valence of arsenic is typically 3-.

(33) Francium has a single valence electron.

(34) Oxygen's valence number in water is -2.

(35) Oxygen's valence number in ozone is -1.

(36) The valence of hydrogen is typically 1+.

(37) The valence of chlorine is typically 1-.

(38) The valence of nitrogen is typically 3-.

(39) The valence of fluorine is typically 1-.

(40) The valence of aluminum is typically 3+.

Valence meaningful sentence

(41) The valence of selenium is typically 2-.

(42) The valence of potassium is typically 1+.

(43) The valence of magnesium is typically 2+.

(44) The valence of tellurium is typically 2-.

(45) Carbon's valence number in methane is -4.

(46) The valence number of gold is typically 3.

(47) The valence number of zinc is typically 2.

(48) The valence of phosphorus is typically 3-.

(49) The valence of gold is typically 1+ or 3+.

(50) Sulfur usually has a valence number of -2.

Valence sentence examples

(51) Alkaline metals have one valence electron.

(52) The valence number of oxygen in water is 2.

(53) Alkaline-earths have two valence electrons.

(54) Oxygen's valence number in peroxides is -1.

(55) Group I elements have one valence electron.

(56) The valence number of oxygen is typically 2.

(57) The valence number of iodine is typically 1.

(58) Phosphorus has a valence number of -3 or +5.

(59) Hydrogen usually has a valence number of +1.

(60) The valence number of oxygen in ozone is -1.

Sentence with valence

(61) The valence number of carbon in methane is 4.

(62) The valence number of carbon in glucose is 4.

(63) The valence number of sulfur in sulfate is 6.

(64) The valence number of bromine is typically 1.

(65) The fluorin atom has seven valence electrons.

(66) Fluorine has a valence of -1 in all compounds.

(67) Calcium has a valence of +2 in most compounds.

(68) Chlorine has a valence of -1 in all compounds.

(69) Nitrogen typically has a valence number of -3.

(70) The valence number of hydrogen in water is +1.

Use valence in a sentence

(71) The valence number of carbon in methane is -4.

(72) The valence number of nitrogen in ammonia is 3.

(73) The valence number of nitrogen in nitrate is 5.

(74) Alkaline metals have a single valence electron.

(75) Hydrogen has a valence of +1 in most compounds.

(76) Aluminum has a valence of +3 in most compounds.

(77) Nitrogen's valence number in nitric acid is +5.

(78) The alkaline-earths have two valence electrons.

(79) Alkali earth metals have two valence electrons.

(80) The tetravalent atom has four valence electrons.

Sentence using valence

(81) Magnesium has a valence of +2 in most compounds.

(82) Sulfur usually has a valence of -2 in compounds.

(83) Oxygen usually has a valence of -2 in compounds.

(84) The valence number of nitrogen in ammonia is -3.

(85) Nitrogen's valence number in ammonium ion is -3.

(86) Alkaline earth metals have two valence electrons.

(87) Alkali earth elements have two valence electrons.

(88) Alkaline-earth-metals have two valence electrons.

(89) The univalent atom had a single valence electron.

(90) Nitrogen usually has a valence of -3 in compounds.

Valence example sentence

(91) The valence number of carbon in acetic acid is +2.

(92) The valence number of phosphorus in phosphate is 5.

(93) The pentavalent element has five valence electrons.

(94) Valence electrons are involved in chemical bonding.

(95) Oxygen's valence number in hydrogen peroxide is -1.

(96) The valence number of sulfur in sulfuric acid is +6.

(97) Chlorine's valence number in hypochlorite ion is -1.

(98) The valence number of nitrogen in nitric acid is +5.

(99) The valence number of chlorine in chlorine gas is 0.

(100) The valence number of phosphorus in phosphine is -3.

Sentence with word valence

(101) The valence number of carbon in carbon dioxide is +4.

(102) The valence of an ion can be determined by its charge.

(103) Hybridization is a key concept in valence bond theory.

(104) The valence number of iron can vary between +2 and +3.

(105) The valence number of sodium in sodium chloride is +1.

(106) The valence number of nitrogen in nitrous oxide is +1.

(107) The valence number of chlorine in sodium chloride is 1.

(108) Oxygen typically has a valence of -2 in most compounds.

(109) Sodium has one valence electron in its outermost shell.

(110) The valence number of sulfur in hydrogen sulfide is -2.

Sentence of valence

(111) Oxygen has six valence electrons in its outermost shell.

(112) The valence number of chlorine in sodium chloride is -1.

(113) The valence number of calcium in calcium chloride is +2.

(114) Valence electrons are the outermost electrons in an atom.

(115) Carbon has four valence electrons in its outermost shell.

(116) Oxygen typically has a valence number of -2 in compounds.

(117) The valence number of magnesium in magnesium oxide is +2.

(118) The valence number of chlorine in hydrochloric acid is -1.

(119) The valence number of hydrogen in hydrogen peroxide is -1.

(120) The valence number of phosphorus in phosphoric acid is +5.

Valence used in a sentence

(121) The valence number of potassium in potassium nitrate is +1.

(122) Divalents are chemical compounds that have a valence of two.

(123) Sodium is an alkali metal and has only one valence electron.

(124) The valence of tin can vary depending on its oxidation state.

(125) The valence electrons of an atom are the outermost electrons.

(126) The valence of iron can vary depending on its oxidation state.

(127) The valence of lead can vary depending on its oxidation state.

(128) Francium has a single valence electron in its outermost shell.

(129) The valence number of iron can vary depending on the compound.

(130) Valence electrons occupy the outermost energy level of an atom.

Valence sentence in English

(131) The valence bond model can explain the concept of bond strength.

(132) The valence of copper can vary depending on its oxidation state.

(133) The valence bond model can explain the concept of bond enthalpy.

(134) Valence bond theory is used to explain the concept of bond order.

(135) The valence of mercury can vary depending on its oxidation state.

(136) Valence electrons are responsible for the conductivity of metals.

(137) The concept of hybrid orbitals is central to valence bond theory.

(138) The valence bond model can predict the bond angles in a molecule.

(139) The valence electrons of an atom occupy the highest energy level.

(140) The valence electrons of an atom determine its chemical behavior.

(141) The chemistry teacher explained the concept of valence electrons.

(142) The valence of antimony can vary depending on its oxidation state.

(143) Valence electrons are involved in the formation of chemical bonds.

(144) The valence electron shell is the highest energy level in an atom.

(145) Valence electrons are involved in the formation of covalent bonds.

(146) Valence electrons are involved in the formation of metallic bonds.

(147) The valence of carbon can vary depending on the compounds it forms.

(148) The valence electron determines the chemical properties of an atom.

(149) Valence bond theory helps in understanding the shapes of molecules.

(150) The valence bond model can predict the strength of a chemical bond.

(151) Valence bond theory is used to explain the concept of bond polarity.

(152) Valence bond theory is used to explain the concept of bond enthalpy.

(153) The concept of resonance can be explained using valence bond theory.

(154) The valence bond approach is widely used in computational chemistry.

(155) Valence bond theory can explain the formation of sigma and pi bonds.

(156) Chalcogen atoms have six valence electrons in their outermost shell.

(157) Divalents are chemical compounds that contain two valence electrons.

(158) The cesium atom has a single valence electron in the outermost shell.

(159) The valence of an atom determines its ability to form chemical bonds.

(160) Valence electrons are crucial in the formation of chemical compounds.

(161) The valence electron shell is the outermost electron shell in an atom.

(162) The valence electron configuration of an atom can affect its stability.

(163) Valence electrons are responsible for the formation of ionic compounds.

(164) The valence bond theory is a fundamental concept in chemical education.

(165) The formation of a positive ion involves the loss of valence electrons.

(166) Carbon dioxide has a valence number of +4 for carbon and -2 for oxygen.

(167) Electrons in the outermost electron shell are called valence electrons.

(168) The valence electron shell can accommodate a maximum of eight electrons.

(169) The valence electron shell is the region where chemical reactions occur.

(170) The valence electrons of an atom can be determined by its atomic number.

(171) Valence bond theory is often used to explain the stability of molecules.

(172) Valence bond theory is often used to explain the concept of bond energy.

(173) The n-s valence electrons of the atom determine its chemical reactivity.

(174) The pentavalent state of an element means it has five valence electrons.

(175) The valence bond model can explain the concept of resonance in molecules.

(176) Valence bond theory is used to explain the concept of bond hybridization.

(177) Valence bond theory is often used in the study of coordination compounds.

(178) The valence bond theory is an alternative to the molecular orbital theory.

(179) Alkaline earth metals have a tendency to lose their two valence electrons.

(180) The formation of an ionic bond involves the transfer of valence electrons.

(181) The valence bond approach is used to explain the concept of bond polarity.

(182) Alkali earth elements have two valence electrons in their outermost shell.

(183) Alkaline-earth metals have two valence electrons in their outermost shell.

(184) Alkaline earth metals have two valence electrons in their outermost shell.

(185) The valence bond model can explain the concept of bond angles in molecules.

(186) Valence electrons are responsible for the formation of molecular compounds.

(187) Alkaline-earths have two valence electrons in their outermost energy level.

(188) The valence electrons of an atom are located in its outermost energy level.

(189) The valence number of an atom determines its ability to form chemical bonds.

(190) The concept of valence bond theory explains the formation of chemical bonds.

(191) Valence bond theory is used to explain the magnetic properties of molecules.

(192) Valence bond theory is often used in predicting the reactivity of molecules.

(193) The noble gases, also called inert gases, have full valence electron shells.

(194) Inert gases are chemically stable due to their full valence electron shells.

(195) In valence bond theory, electrons are localized between two atoms in a bond.

(196) Valence bond theory is used to explain the stability of noble gas compounds.

(197) The number of valence electrons determines an element's chemical properties.

(198) The valence bond model can explain the phenomenon of resonance in molecules.

(199) The valence bond approach considers the electron pairs as localized entities.

(200) Valence bond theory provides a qualitative understanding of chemical bonding.

(201) Valence electrons are responsible for the color and conductivity of elements.

(202) Valence bond theory can explain the concept of bond length and bond strength.

(203) Alkali metals have a single valence electron in their outermost energy level.

(204) Valence bond theory helps in understanding the concept of bond hybridization.

(205) Valence bond theory can explain the formation of multiple bonds between atoms.

(206) The valence electrons of an atom determine its position in the periodic table.

(207) The valence electrons of an atom are responsible for its ability to form ions.

(208) The valence electrons of an atom can be found in the outermost electron shell.

(209) The valence bond model can explain the stability of molecules and their shapes.

(210) Valence bond theory is used to explain the concept of bond dissociation energy.

(211) Valence bond theory is used to explain the concept of molecular orbital theory.

(212) The alkaline-earths have two valence electrons in their outermost energy level.

(213) Valence bond theory predicts the geometry and magnetic properties of molecules.

(214) Sodium is an electropositive element that readily donates its valence electron.

(215) The valence electrons are responsible for the chemical reactivity of an element.

(216) Valence bond theory can explain the stability of molecules and their reactivity.

(217) The valence bond approach is used to describe the bonding in diatomic molecules.

(218) Valence bond theory is a useful tool for predicting the reactivity of molecules.

(219) The isoelectronic series of atoms all have the same number of valence electrons.

(220) The valence bond model can explain the formation of multiple bonds between atoms.

(221) Valence bond theory is a fundamental concept in understanding chemical reactions.

(222) Alkaline earth metals have two valence electrons in their outermost energy level.

(223) Valence bond theory is based on the idea that electrons occupy specific orbitals.

(224) The valence bond approach is used to explain the reactivity of organic compounds.

(225) The valence electrons of an atom are involved in the formation of chemical bonds.

(226) The valence electrons of an atom are responsible for its electrical conductivity.

(227) The valence electrons of an atom are crucial in determining its bonding patterns.

(228) Electrovalency is influenced by the number of valence electrons an atom possesses.

(229) The valence bond model predicts the geometry and magnetic properties of molecules.

(230) The valence bond model can explain the paramagnetic behavior of certain compounds.

(231) The valence electrons of an atom can be represented by the electron dot structure.

(232) Bivalences can be used to determine the valence electron configuration of an atom.

(233) Valence bond theory is a key concept in understanding the nature of chemical bonds.

(234) The valence bond model can explain the concept of bond formation and bond breaking.

(235) The valence bond approach considers the concept of sigma and pi bonds in molecules.

(236) The formation of an ionic bond involves the complete transfer of valence electrons.

(237) The valence bond approach provides a qualitative understanding of chemical bonding.

(238) The valence bond model can be used to explain the hybridization of atomic orbitals.

(239) Valence bond theory helps in understanding the concept of bond angles in molecules.

(240) Valence bond theory describes the overlapping of atomic orbitals in a covalent bond.

(241) The metallic bond is stronger in metals with higher valence electron concentrations.

(242) The valence bond approach is used to explain the concept of electron delocalization.

(243) The valence bond model can explain the formation of sigma and pi bonds in molecules.

(244) The valence bond approach considers the overlapping of atomic orbitals to form bonds.

(245) The valence bond model is used to describe the bonding in transition metal complexes.

(246) The valence bond approach is particularly useful for understanding organic chemistry.

(247) The valence bond model can predict the magnetic properties of coordination compounds.

(248) The valence electrons of an atom can be represented by dots in a Lewis dot structure.

(249) Valence bond theory helps in understanding the strength and length of chemical bonds.

(250) The valence bond approach considers the electron configuration of atoms in a molecule.

(251) The valence bond approach is based on the idea of electron pairing in chemical bonding.

(252) Valence electrons can be transferred or shared between atoms during chemical reactions.

(253) Tetravalency is a result of the outermost electron shell having four valence electrons.

(254) The valence bond approach is used to explain the concept of bond length and bond energy.

(255) The valence bond approach considers the concept of electron delocalization in molecules.

(256) The number of valence electrons in an atom can be used to predict its chemical behavior.

(257) The valence electrons of an atom can be shared or transferred during chemical reactions.

(258) The valence electrons of an atom are responsible for its ability to conduct electricity.

(259) Valence bond theory helps in understanding the concept of bond strength and bond length.

(260) The valence electron configuration of an atom can be used to determine its atomic radius.

(261) The valence electrons of an atom can be shared between multiple atoms in a covalent bond.

(262) Valence bond theory provides a basis for understanding the concept of molecular orbitals.

(263) Valence bond theory provides a framework for understanding the strength of chemical bonds.

(264) Valence bond theory is used to explain the concept of bond polarity and electronegativity.

(265) Halogens are located in group 17 of the periodic table, and they have 7 valence electrons.

(266) The reactivity of an element is determined by the number of valence electrons it possesses.

(267) The valence electron configuration of an atom can be used to determine its oxidation state.

(268) The valence electron configuration of an atom can be used to determine its Lewis structure.

(269) The valence electrons of an atom can be represented by the electron configuration notation.

(270) The valence electrons of an atom can be visualized as the electrons in the outermost shell.

(271) The valence bond approach provides a framework for understanding the concept of bond order.

(272) The valence electron configuration of an atom can be used to determine its chemical formula.

(273) The valence electrons of an atom play a crucial role in determining its chemical reactivity.

(274) Halogens, which are located in Group 17 of the periodic table, have seven valence electrons.

(275) The valence electron configuration of an atom can be represented using electron dot diagrams.

(276) The valence electron configuration of an atom can be used to predict its chemical reactivity.

(277) The valence electron configuration of an atom can be used to determine its electronegativity.

(278) The valence electron configuration of an atom can be used to determine its ionization energy.

(279) Tetravalency is a property that is influenced by the number of valence electrons an atom has.

(280) The ionizing energy of an atom can be affected by the presence of multiple valence electrons.

(281) The valence electrons of an atom can be determined by its group number on the periodic table.

(282) In valence bond theory, the valence electrons of atoms are localized in overlapping orbitals.

(283) The valence bond approach is used to explain the concept of bond formation and bond breaking.

(284) In a metallic bond, the valence electrons are shared among all the atoms in the metal lattice.

(285) The valence electron configuration of an atom can be used to determine its magnetic properties.

(286) Valence bond theory is a fundamental concept in understanding the nature of chemical compounds.

(287) The electrovalency of an atom can be determined by the number of valence electrons it possesses.

(288) Valence bond theory is a key concept in understanding the structure and properties of molecules.

(289) In a metal, the valence electrons become free electrons and move freely throughout the material.

(290) Valence bond theory provides a framework for understanding the bonding in coordination compounds.

(291) The valence bond approach is based on the idea that electrons are localized around atomic nuclei.

(292) Valence bond theory is a fundamental concept in understanding the concept of chemical reactivity.

(293) The valence electrons of an atom are involved in the formation of chemical bonds with other atoms.

(294) The formation of an ionic bond involves the transfer of valence electrons from one atom to another.

(295) Valence bond theory is a key concept in understanding the properties of transition metal complexes.

(296) The valence bond model can explain the phenomenon of electron delocalization in conjugated systems.

(297) Alkaline metals are found in group 1 of the periodic table, and they all have one valence electron.

(298) Photoelectron spectroscopy provides valuable information about the valence band structure of solids.

(299) Valence bond theory is a useful tool for understanding the reactivity of transition metal complexes.

(300) Alkali metals are highly reactive because they have a strong tendency to lose their valence electron.

(301) The concept of valence bond theory explains chemical bonding in terms of overlapping atomic orbitals.

(302) The valence electron configuration of an atom can be determined by its position in the periodic table.

(303) The valence electron configuration of an atom can be used to determine its melting and boiling points.

(304) Valence electrons play a crucial role in determining the physical and chemical properties of elements.

(305) Valence bond theory suggests that covalent bonds are formed by the overlap of valence atomic orbitals.

(306) The number of valence electrons in an atom can be determined by its group number on the periodic table.

(307) The valence bond model describes the formation of chemical bonds through the sharing of electron pairs.

(308) The valence bond approach provides a framework for understanding the electronic structure of molecules.

(309) The valence bond model predicts the geometry of molecules based on the hybridization of atomic orbitals.

(310) The valence electron shell is the most important factor in determining the chemical behavior of an atom.

(311) The eigenfrequency of the electron in the atom's valence shell determines its chemical bonding behavior.

(312) Alkaline-earths are a group of elements found in the periodic table, and they have two valence electrons.

(313) The strength of a metallic bond depends on the number of valence electrons and the size of the metal atoms.

(314) The valence bond approach is based on the idea that electrons occupy specific regions of space around atoms.

(315) Psychophysics experiments often involve participants making judgments about the emotional valence of a stimulus.

(316) Alkaline-earths, which have a low electronegativity, readily lose their valence electrons to form positive ions.

(317) Alkaline-earths, which have a low ionization energy, readily lose their valence electrons to form positive ions.

(318) Sodium is an alkali metal, which means it has a single valence electron that is easily lost in chemical reactions.

(319) The formal charge of an atom can be calculated by comparing its valence electrons with its actual number of electrons.

(320) The formal charge of a covalent bond can be calculated by subtracting the shared electrons from the valence electrons.

(321) The valence electrons of an atom can be calculated by subtracting the core electrons from the total number of electrons.

(322) The band gap of a material determines the energy required for an electron to transition from the valence band to the conduction band.

(323) The formal charge of the molecule can be calculated by subtracting the number of valence electrons from the number of electrons in the molecule.

(324) The formal charge of an atom can be calculated by subtracting the number of valence electrons from the number of lone pair electrons and half the number of bonding electrons.

(325) The law of definite proportions is a consequence of the fact that atoms combine in fixed ratios to form molecules, and these ratios are determined by the valence of the atoms involved.

(326) The formal charge of the central atom in a molecule can be calculated by subtracting the number of valence electrons from the sum of the lone pair electrons and half the bonding electrons.

The word usage examples above have been gathered from various sources to reflect current and historical usage of the word Valence. They do not represent the opinions of TranslateEN.com.