Chemistry

all digits of a measured quantity, including the uncertain one! significant figures- solids have a definite shape & volume, liquids have a definite volume, and gas has neither! matter classification (look at charts in notes)- can be observed without changing the identity and composition of the substance (phase change)! physical properties- describe the way a …

copper (I) chloride CuCl mercury (II) oxide HgO iron (III) oxide Fe₂O₃ manganese (IV) oxide MnO₂ lead (IV) chloride PbCl₄ cobalt (II) bromide CoBr₂ chromium (III) chloride CrCl₃ lead (II) bromide PbBr₂ lead (IV) bromide PbBr₄ iron (II) sulfide FeS iron (III) sulfide Fe₂S₃ cobalt (III) chloride CoCl₃ copper (II) oxide CuO titanium (IV) chloride …

Group 1 has ⁺¹ Charge. (Li, Na, K, Rb, Cs) Group 2 has ⁺² Charge. (Mg, Ca, Sr, Ba) Other is diagonal on the periodic table (Ag⁻¹, Zn⁺², Cd⁺², Al⁺³) Monoatomic Ions (Cations) Group 17 has ⁻¹ Charge. (F, Cl, Br, I) Group 16 has ⁻² Charge. (O, S Se, Te) Group 15 has ⁻³ …

NO₃⁻ Nick BrO₃⁻ Brit CO₃²⁻ Camel IO₃⁻ Inch ClO₃⁻ Clam CrO₄²⁻ Crepes SO₄²⁻ Supper PhO₄³⁻ Phoenix +1 per___ate ___ate -1 ___ite -2 hypo___ite

Hg2 2+ Mercury(I) NH4 + Ammonium NO2 – Nitrite NO3 – Nitrate SO3 2- Sulfite SO4 2- Sulfate HSO4 – Hydrogen Sulfate (Bisulfate) OH – Hydroxide CN – Cyanide PO4 3- Phosphate HPO4 2- Hydrogen Phosphate H2PO4 – Dihydrogen Phosphate SCN – Thiocyanate CO3 2- Carbonate HCO3 – Hydrogen Carbonate (Bicarbonate) ClO – Hypochlorite ClO2 …

H+. 1+ monatomic ion Hydrogen Li+. 1+ monatomic ion Lithium Na+. 1+ monatomic ion Sodium K+. 1+ monatomic ion Potassium Rb+. 1+ monatomic ion Rubidium Cs+. 1+ monatomic ion Cesium Ag+. 1+ monatomic ion Silver Be2+. 2+ monatomic ion Berylium Mg2+. 2+ monatomic ion Magnesium Sr2+. 2+ monatomic ion Strontium Ba2+. 2+ monatomic ion Barium …

# of Oxygen consonants charge # (-) vowels NO – 3 Nick BrO – 3 Baby CO 2- 3 Camel IO – 3 Inch ClO – 3 Clam SO 2- 4 Supper PO 3- 4 Phoenix Nick the Camel ate an Inch Clam for Supper in Phoenix. What is the whole sentence?

NO3 – nitrate NO2 – nitrite CO3 2- carbonate HCO3 – bicarbonate ClO3 – chlorate ClO2 – chlorite ClO – hypochlorate ClO4 – perchlorate SO4 2- sulfate SO3 2- sulfite HSO4 – bisulfate PO4 3- phosphate HPO4 2- biphosphate H2PO4 – dihydrogen phosphate CN – cyanide OH – hydroxide CH3COO – acetate NH4 + ammonium …

Ammonium ion NH4+ Hydroxide ion OH- Cyanide ion CN- Nitrite ion NO2- Nitrate ion NO3- Thiocyanate ion SCN- Acetate ion C2H4O2- (CH3COOH-) Hypochlorite ion CIO- Chlorite ion CIO2- Chlorate Ion CIO3- Perchlorate ion CIO4- Bicarbonate ion (Hydrogen Carbonate) HCO3- Bromate ion BrO3- Permanganate ion MnO4- Carbonate ion CO23- Oxalate ion C2O42- Chromate ion CrO42- Dichromate …

NO₃⁻¹ Nitrate = Nick (3 consonants and 1 vowel) NO₂⁻¹ Nitrite = little Nick (one less consonant) CO₃⁻² Carbonate = Camel (3 consonants and 2 vowels) O₂⁻² Peroxide = bleached little camel wigy (visualize) (Only Oxygen wigy= 2 consonants and 2 vowels) ClO₃⁻¹ Chlorate = Clam (3 consonants and 1 vowel) ClO₂⁻¹ chlorite = little …

ionic compound metal + nonmetal Arise from transfer of the electrons from the metal to nonmetal. ionic compounds positively charged Metals in an ionic compound become? (+/-) negatively charged Nonmetals in an ionic compound become? (+/-) name of metal (as is) + name of nonmetal ending in “ide” ex: aluminum sulfide Binary compounds naming Group …

Metals->Nonmetals No charge in formula Ionic compounds are consisted of The charge on the ion Roman numerals in name of ionic compounds represent what Add -ide suffix Add what to ionic compounds Always neutral Ionic Compounds are what Ionic compounds that’s for multiple ions Roman numerals are In what name Nonmetals->Nonmetals Polyatomic ions are consisted …

1- What is the change of an ion with 6 protons and 7 electrons? 2- An atom gains two electrons to form an ion. What is the charge of this ion? 1- What is the charge of an ion formed from an element with the electron configuration 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁵? The atomic radius of Na is larger …

ammonium NH₄⁺ nitrate NO₃⁻ sulfate SO₄²⁻ hydroxide OH⁻ cyanide CN⁻ phosphate PO₄³⁻ carbonate CO₃²⁻ methane CH₄ ammonia NH₃⁺ Dissolved in water Soluable/aqueous H,O,N,F,Cl,Br,I Diatomic Elements Phosphorus (Tetratomic) P₄ Sulfur (Octatomic) S₈ Name for the normal, balanced equation Non-ionic equation Spectator IonWhen writing a net ionic equation, these ions found in the original equation are removed. …

Add up all valence electrons in the molecule Lewis dot structure rule 1 Place the least electronegative atom in the center. H never goes in the middle; oxygen rarely; carbon almost always L.D.S. Rule 2 Place the remaining atoms symmetrically around the center L.D.S. Rule 3 Use lines to connect atoms LDS rule 4 Place …

Ammonium NH4+ Acetate C2H3O2- Carbonate CO3^2- Hypochlorite ClO- Chlorite CIO2- Chlorate ClO3- Perchlorate ClO4- Cyanide CN- Hydroxide OH- Nitrite NO2- Nitrate NO3- Permanganate MnO4- Phosphite PO3^3- Phosphate PO4^3- Sulfite SO3^2- Sulfate SO4^2-

An ionic bond results from electrical attraction between cations and anions. A non-polar covalent bond is unlikely when two atoms of different elements join because the atoms are likely to differ in electronegativity Bond length is the distance between two bonded atoms at their minimum potential energy. to draw a Lewis structure, it is not …

When the metals in Groups 1A, 2A, and 3A lose electrons, they form cations with positive charges equal to their group number. The charge of any ion of a Group A nonmetal is determined by subtracting 8 from the group number. Explain how the charges of Group A metal and nonmetal ions are related to …

multivalent more than one ion form cation Roman numeral are used after the which ion was used Roman numeral are used to indicate ide two atoms usually has an “___” ending ide monatomic atoms usually has an “___” ending oxygen “per” usually indicates an extra “ate” If there are several combinations The commonest ion ends …

ammonium NH4+ nitrite NO2- nitrate NO3- sulfite SO32- sulfate SO42- hydrogen sulfate (bisulfate) HSO4+ hydroxide OH- cyanide CN- phosphate PO43- hydrogen phosphate HPO42- dihydrogen phosphate H2PO4- carbonate CO32- hydrogen carbonate (bicarbonate) HCO3- hypochlorite ClO- chlorite ClO2- chlorate ClO3- perchlorate ClO4- acetate C2H3O2- permanganate MnO4- dichromate Cr2O72- chromate CrO42- peroxide O22-

Compounds containing three or more elements (at least one polyatomic ion) Ternary Compounds An ionic compound that is composed of cations bonded to anions , other than oxide or hydroxide ions Salt Cation than anion Na3PO4 = Sodium phosphate Rules for naming Compounds with polyatomic ions Roman Numerals Fe(NO3)2 = Iron (II) Nitrate Transition metals …

Cation, Anion Binary ionic compounds are named by writing the name of the ______ followed by the name of the _____. -ide Names of binary compounds end in ______. Sodium Iodine For example, NaI is ______. Roman Numeral When a cation has more that one ionic charge, a _____ is used in the name. Anion, …

Cu + Copper (I) ion Cu 2+ Copper (II) ion Fe 2+ Iron (II) ion Fe 3+ Iron (III) ion Hg2 2+ Mercury (I) ion Hg 2+ Mercury (II) ion Pb 2+ Lead (II) ion Pb 4+ Lead (IV) ion Sn 2+ Tin (II) ion Sn 4+ Tin (IV) ion Cr 2+ Chromium (II) ion …

when they are bonded to other atoms When do most atoms have lower potential energy? attract In the formation of a Covalent bond, the electrons of one atom and the protons of the other atom ______ one another? repel In the formation of a Covalent bond, Two Nuclei and two electrons ________ each other? either …

Noble gases These don’t combine with other atoms Pure substance, composed of two or more elements with a definite composition Compound Ionic or covalent 2 types of compounds One or more electrons are transferred from the atoms of metals to atoms of nonmetals Ionic compound (what happens with electrons?) The cations and anions have different …