Biology

C. the valence electrons In an electron-dot structure of an element, the dots are used to represent In an electron-dot structure of an element, the dots are used to represent A. the electrons that the element will gain when it forms a compound. B. only the electrons that will participate in bond formation. C. the …

*+1* *+1* Ammonium *+2* *+2* Dimercury *-1* *-1* Acetate Bromate Chlorate Chlorite Cyanide Dihydrogen phosphate Hydrogen Carbonate (bicarbonate) Hydrogen sulfate Hydroxide Hypochlorite Nitrate Nitrite Perchlorate Permanganate *-2* *-2* Carbonate Chromate Dichromate Hydrogen phosphate Oxalate Peroxide Sulfate Sulfite *-3* *-3* Arsenate Phosphate

structural formula a depiction of the arrangement of atoms in molecules and polyatomic ions single covalent bond a covalent bond in which only one pair of electrons is shared double covalent bond a covalent bond in which two pairs of electrons are shared coordinate covalent bond a covalent bond in which the shared electron pair …

True. True or false? In naming ionic compounds, the cation is always named first and the anion second. . H2S 2. Which of the following is a binary compound? lithium chloride The correct name for LiCl is mercury(I) ion The name for Hg22+ is . iron(II) oxide The correct name for FeO is +2 The …

ammonium NH4+ nitrite NO2- nitrate NO3- sulfite SO3^2- sulfate SO4^2- hydrogen sulfate HSO4- hydroxide OH- cyanide Cn- phosphate PO4^3- hydrogen phosphate HPO4^2- dihydrogen phosphate H2PO4- carbonate CO3^2- hydrogen carbonate HCO3- hypochlorite CLO- chlorite CLO2- chlorate CLO3- perchlorate CLO4- acetate C2H3O2 dichromate Cr2O7^2- chromate CrO4^2- peroxide O2^2-

H₃O⁺ Hydronium Hg₂²⁺ Dimercury (1) NH₄⁺ Ammonium C₂H₃O₂⁻, CH₃COO⁻ Acetate CN⁻ Cyanide CO₃²⁻ Carbonate HCO₃⁻ Hydrogen Carbonate C₂O₄²⁻ Oxalate ClO⁻ Hypochlorite ClO₂⁻ Chlorite ClO₃⁻ Chlorate ClO₄⁻ Perchlorate CrO₄²⁻ Chromate Cr₂O₇²⁻ Dichromate MnO₄⁻ Permanganate NO₂⁻ Nitrite NO₃⁻ Nitrate O₂²⁻ Peroxide OH⁻ Hydroxide PO₄³⁻ Phosphate SCN⁻ Thiocyanate SO₃²⁻ Sulfite SO₄²⁻ Sulfate HSO₄⁻ Hydrogen Sulfate S₂O₃²⁻ Thiosulfate

monatomic ion Consists of a single atom with a positive or negative charge anion atom or group of atoms having a negative charge cation atom or group of atoms having a positive charge polyatomic ion tightly-bound group of atoms that behaves as a unit and carries a net charge binary compound compound composed of two …

H2PO-1 Dihydrogen phosphate C2H3O2-1 Ethanoate HSO3-1 Hydrogen sulfite HSO4-1 Hydrogen sulfate HCO3-1 Hydrogen carbonate NO2-1 Nitrite NO3-1 Nitrate CN-1 Cyanide OH-1 Hydroxide MnO4-1 Permanganate ClO-1 Hypochlorite ClO2-1 Chlorite ClO3-1 Chlorate ClO4-1 Perchlorate HPO4-2 Hydrogen phosphate C2O4-2 Oxalate SO3-2 Sulfite SO4-2 Sulfate CO3-2 Carbonate CrO4-2 Chromate Cr2O7-2 Dichromate SiO3-2 Silicate PO3-3 Phosphite PO4-3 Phosphate NH4+ Ammonium

atoms lose, gain, or share valence electrons to have 8 valence electrons. The octet rule indicates that metals, cations In ionic compounds ________ lose their valence electrons to form positively charged ________. lose 3 How many electrons will aluminum gain or lose when it forms an ion? K+ What is the symbol for the ion …

base produces a hydroxide ion when dissolved in water law of definite proportions in any chemical compound, the masses of elements are always in the same proportion by mass polyatomic ion tightly-bound group of atoms that behaves as a unit and carries a net charge anion atom or group of atoms having a negative charge …

NH₄OH Ammonium Hydroxide NaOH Sodium Hydroxide KOH Potassium Hydroxide LiOH Lithium Hydroxide RbOH Rubidium Hydroxide Ca(OH)₂ Calcium Hydroxide Mg(OH)₂ Magnesium Hydroxide Sr(OH)₂ Strontium Hydroxide Al(OH)₃ Aluminium Hydroxide Be(OH)₂ Beryllium Hydroxide NH₄CN Ammonium Cyanide NaCN Sodium Cyanide KCN Potassium Cyanide LiCN Lithium Cyanide RbCN Rubidium Cyanide Ca(CN)₂ Calcium Cyanide Mg(CN)₂ Magnesium Cyanide Sr(CN)₂ Strontium Cyanide Al(CN)₃ …

phosphate PO₄³⁻ hydrogen phosphate HPO₄²⁻ dihydrogen phosphate H₂PO₄⁻ phosphite PO₃³⁻

The major assumption is that pairs of valence electrons repel each other. Identify the major assumption of the VSEPR theory, which is used to predict the shape of atoms. The lone pairs of electrons on oxygen make the molecular shape bent or angular. In water, two hydrogen atoms are bonded to one oxygen atom. Why …

NO₃⁻ nitrate SO₄²⁻ sulfate PO₄³⁻ phosphate CO₃²⁻ carbonate C₂H₃O₂⁻ acetate OH⁻ hydroxide ClO₃⁻ chlorate NH₄⁺ ammonium one more oxygen than –ate per–ate one less oxygen than –ate –ite two less oxygen than –ate hypo–ite mono 1 bi 2 tri 3 tetra 4 penta 5 hexa 6 hepta 7 octa 8 nona 9 deca 10 write …

NO₃⁻ Nitrate ClO₃⁻ Chlorate OH⁻ Hydroxide CO₃⁻² Carbonate SO₄⁻² Sulfate PO₄⁻³ Phosphate NH₄⁺ Ammonium

NH4+ ammonium NO3- nitrate SO4-2 sulfate OH− hydroxide PO4-3 phosphate CO3-2 carbonate C2H3O2- acetate

5)electrons are lost and the ion is smaller When a cation is formed from a representative element 1)electrons are gained and the ion is larger. 2)electrons are lost and the ion is larger. 3)electrons are gained and the ion is smaller. 4)the cation acquires a negative charge. 5)electrons are lost and the ion is smaller …

a covalent bond in which the shared electron pair comes form only one of the atoms coordinate covalent bond a covalent bond in which two pairs of electrons are shared Double Covalent bond A depiction of the arrangement of atoms in molecules and polyatomic ions Structural formula A covalent bond in which only one pair …

-color change -formation of a solid -formation of gas -emission of light -emission or absorption of heat What are the main indicators that a chemical reaction has occurred? -g: gas -l: liquid -s: solid -aq: aqueous What does each abbreviation, often used in chemical equations, represent? g, I, s, aq -a homogeneous mixture of a …

Aluminum Phosphate AlPO4 Potassium Nitrite KNO2 Sodium Bicarbonate NaHCO3 Calcium Carbonate CaCO3 Magnesium Hydroxide Mg(OH)2 Sodium Chromate Na2CrO4 Barium Cyanide Ba(CN)2 Potassium Sulfate K2SO4 Sodium Dibiphosphate NaH2PO4 Ammonium nitrate NH4NO3 Tin (II) Nitrate Sn(NO3)2 Iron (III) Phosphate FePO4 Copper Sulfate Cu2SO4 Nickel Acetate Ni(C2H3O2)s Mercury Carbonate HgCO3) Lead Hydroxide Pb(OH)4 Copper Dichromate Cu2Cr2O7 Copper (II) …

Roman Numeral following the name When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a ____. tin (II) phosphate What is the correct name for Sn(3)(PO4)(2) nitride ion What is the correct name for the N(3)- ion. tin (IV) fluoride, …

dihydrogen phosphate H₂PO₄⁻ acetate C₂H₃O₂⁻ cyanate OCN⁻ hydrogen sulfite (bisulfate) HSO₃⁻ hydrogen sulfate (bisulfate) HSO₄⁻ Hydrogen carbonate (bicarbonate) HCO₃- nitrite NO₂⁻ Nitrate NO₃⁻ Cyanide CN⁻ hydroxide OH⁻ Permanganate MnO₄⁻ Hypochlorite ClO⁻ Chlorite ClO₂⁻ Chlorate ClO₃⁻ perchlorate ClO₄⁻ Thiocyanate SCN⁻ Hydrogen Phosphate HPO₄²⁻ Peroxide O₂²⁻ Oxalate C₂O₄²⁻ Thiosulfate S₂O₃²⁻ sulfite SO₃²⁻ Sulfate SO₄²⁻ Carbonate CO₃²⁻ Chromate …

NH₄¹⁺ AMMONIUM Hg₂²⁺ MERCURY PH₄¹⁺ PHOSPHONIUM C₂H₃O₂¹⁻ ACETATE N₃¹⁻ AZIDE BrO₃¹⁻ BROMATE BrO₂¹⁻ BROMITE ClO₃¹⁻ CHLORATE ClO₂¹⁻ CHLORITE CN¹⁻ CYANIDE H₂PO₄¹⁻ DIHYDROGEN PHOSPHATE H¹⁻ HYDRIDE HCO₃¹⁻ HYDROGEN CARBONATE (bicarbonate) HSO₄¹⁻ HYDROGEN SULFATE (bisulfate) HS¹⁻ HYDROGEN SULFIDE (bisulfide) HSO₃¹⁻ HYDROGEN SULFITE (bisulfite) OH⁻¹ HYDROXIDE BrO¹⁻ HYPOBROMITE ClO¹⁻ HYPOCHLORITE IO¹⁻ HYPOIODITE IO₃¹⁻ IODATE IO₂¹⁻ IODITE NO₃¹⁻ NITRATE …

C₂H₃O₂¹⁻ or CH₃COO¹⁻ Acetate NH₂¹⁻ Amide NH₄¹⁺ Ammonium BrO₃¹⁻ Bromate BrO₂¹⁻ Bromite CO₃²⁻ Carbonate ClO₃¹⁻ Chlorate ClO₂¹⁻ Chlorite CrO₄²⁻ Chromate CN¹⁻ Cyanide Cr₂O₇²⁻ Dichromate H₂PO₄¹⁻ Dihydrogen Phosphate HCO₃¹⁻ Hydrogen Carbonate (Bicarbonate) HPO₄²⁻ Hydrogen Phosphate HSO₄¹⁻ Hydrogen Sulfate (Bisulfate) HSO₃¹⁻ Hydrogen Sulfite (Bisulfite) H₃O¹⁺ Hydronium OH¹⁻ Hydroxide BrO¹⁻ Hypobromite ClO¹⁻ Hypochlorite IO¹⁻ Hypoiodite IO₃¹⁻ Iodate IO₂¹⁻ …

C) Hg 1) The symbol for the element mercury is_. A) Pb B) Sn C) Hg D) Me C) solutions 2) Homogeneous mixtures are also known as_. A) substances B) elements C) solutions D) solids E) compounds B) 1.3 x 10^3 g. 3) Iron has a density of 7.9 g/cm3. What is the mass of …