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Quiz 2 study help
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1Dalton's atomic theory:
All [blank_start]matter[blank_end] is composed of [blank_start]atoms[blank_end].
[blank_start]Atoms are[blank_end] very small particles of matter that retain their identity during chemical reactions.
Atoms [blank_start]cannot[blank_end] be subdivided and maintain their distinct characteristics.
Atoms [blank_start]combine[blank_end] to form elements and all the atoms of the element have identical properties such as a definite mass.
[blank_start]Elements[blank_end] combine to form compounds that are represented by simple whole-number ratios.
Atoms are not [blank_start]created, destroyed, or decomposed[blank_end] during a chemical process- Amatter
- Batoms
- CAtoms are
- Dcannot
- Ecombine
- FElements
- Gcreated, destroyed, or decomposed
2[blank_start]Atomic symbols[blank_end] are one or two-letter notation(s) representing an atom of a particular element. The first letter is capitalized followed by lower case letters. Some symbols are derived from a Latin nomenclature
- AAtomic symbols
- BChemical symbols
- CElemental symbols
3[blank_start]The Law of Conservation of Mass[blank_end] says: the total mass of materials remains constant during a chemical reaction and atoms are not created or destroyed during the chemical reaction.
Atoms have [blank_start]definite mass[blank_end]; therefore, compounds contain elements in definite proportions by mass.
The masses of one element which combine with a fixed mass of the second element are in a ratio of [blank_start]small whole numbers[blank_end].- AThe Law of Conservation of Mass
- Bdefinite mass
- Csmall whole numbers
- Dsmall numbers
- Eindefinite mass
4Atoms are made up of very small particles (referred to as subatomic particles). The center (nucleus) of the atom consists of [blank_start]protons, positively charged particles[blank_end], and [blank_start]neutrons, particles with zero charge[blank_end]. [blank_start]Electrons, negatively charged particles[blank_end], are in an orbit of sorts around the nucleus.
- Aprotons, positively charged particles
- Bneutrons, particles with zero charge
- CElectrons, negatively charged particles
5[blank_start]Isotopes[blank_end] are atoms with the same [blank_start]atomic number, Z,[blank_end] but different [blank_start]atomic masses, A[blank_end]. This means that [blank_start]isotopes[blank_end] have the same number of [blank_start]protons[blank_end], but a different number of [blank_start]neutrons[blank_end].
- AIsotopes
- Batomic number, Z,
- Catomic masses, A
- Disotopes
- Eprotons
- Fneutrons
6[blank_start]Atomic mass[blank_end] is the average mass for the naturally occurring elements. [blank_start]Protons[blank_end] and [blank_start]neutrons[blank_end] weigh [blank_start]1 AMU (atomic mass unit)[blank_end].
- AAtomic mass
- BProtons
- Cneutrons
- Delectrons
- EElectrons
- Fpositrons
- G1 AMU (atomic mass unit)
- H2 AMU (atomic mass units)
7In 1860, Dmitri Mendeleev and J. Lothar Meyer independently arranged the elements in order of their [blank_start]atomic masses[blank_end]. The elements were arranged in horizontal rows so that elements in vertical columns had similar properties. This arrangement of elements was referred to as the periodic table. Today, the elements are arranged as a periodic function of their [blank_start]atomic number[blank_end].
- Aatomic masses
- Batomic number
8 [blank_start]Metals[blank_end]:
have luster
conduct heat and electricity
are solids at room temperature (except Hg which is a liquid at room temperature)
malleable (capable of transforming into another shape by beating with a hammer or rollers) and ductile ( capable of being drawn out into wire or thread)
[blank_start]Metalloids[blank_end]:
are semi-metallic, i.e., they have [blank_start]metallic and nonmetallic[blank_end] properties
are semiconductors (good conductors of electricity at high temperatures)
[blank_start]nonmetals[blank_end] are:
gases or solids, and bromine is the only liquid
solids are hard and brittle- AMetals
- BMetalloids
- Cmetallic and nonmetallic
- Donly some metallic properties
- Eonly some nonmetal properties
- Fnonmetals
9[blank_start]Chemical[blank_end] formulas give the relative proportions of atoms of different elements in a substance. A [blank_start]molecule[blank_end] is a group of atoms that are [blank_start]chemically bonded[blank_end]. [blank_start]Molecular[blank_end] formulas contain the exact number of different atoms of an element in a molecule. [blank_start]Structural[blank_end] formulas show how atoms are bonded to one another in a molecule.
- AChemical
- BMolecular
- Cmolecule
- Dchemically bonded
- Ephysically combined
- FStructural
10[blank_start]Ions[blank_end] are electrically charged particles that are obtained by removing or adding [blank_start]electrons[blank_end] to an atom or molecule.
An [blank_start]anion[blank_end] is a negatively charged ion.
A [blank_start]cation[blank_end] is a positively charged ion.- AIons
- Belectrons
- Cprotons
- Dneutrons
- Eanion
- Fcation
11When writing [blank_start]ionic[blank_end] compounds, crisscross the charges making sure that each element has been multiplied by the crisscross factor.
- Aionic
- Bcovalent
- Corganic
12[blank_start]Organic[blank_end] compounds are compounds that contain carbon multiply bonded to other carbon atoms. Seventy (70) percent of all registered compounds are [blank_start]organic[blank_end] compounds. The simplest [blank_start]organic compounds[blank_end] contain only carbon and hydrogen and are referred to as hydrocarbons. [blank_start]Organic compounds[blank_end] can also be classified as alcohols, ethers, acids, amines, and an array of other types of compounds depending on the major functional group that identifies the compound.
- AOrganic
- Bcovalent
- Corganic
- DCovalent
- Eorganic compounds
- Fcovalent compounds
- GOrganic compounds
- HCovalent compounds
13When naming [blank_start]Ionic[blank_end] compounds, remember [blank_start]Ionic compounds[blank_end] are made up of a [blank_start]metal[blank_end] cation and a [blank_start]nonmetal[blank_end] anion. The [blank_start]cation[blank_end] is named first followed by the name of the [blank_start]anion[blank_end].
- AIonic
- Borganic
- Ccovalent
- DIonic compounds
- Ecovalent compounds
- FOrganic compounds
- Gmetal
- Hnonmetal
- Ication
- Janion
14Most metals in the Periodic Table, have one [blank_start]monoatomic[blank_end] cation with a charge equal to the [blank_start]Group number[blank_end]. Most transition elements (Groups 8, 9, and 10 or Groups IIIB-IIB of periods 4, 5, 6) in the Periodic Chart, form more than one monatomic cation with different charges.
- Amonoatomic
- BGroup number
- Catomic number
- Datomic mass
- Echarge
15Monoatomic [blank_start]cations[blank_end] are named after the element, e.g., Na+1 is sodium ion. If [blank_start]the cation[blank_end] has more than one charge, a Roman numeral in parentheses is used to designate the charge. Monatomic [blank_start]anions[blank_end] are named by using the stem name of the element and “ide,”.[blank_start]Polyatomic ions[blank_end] are ions that consist of two or more elements chemically combined that function as a single unit.
- Acations
- Bthe cation
- Cthe anion
- Danions
- EPolyatomic ions
- FCompounds
16[blank_start]Binary compounds[blank_end] are compounds composed of two elements. [blank_start]Ionic binary compounds[blank_end] are composed of a metal cation and a nonmetal anion and are held together by [blank_start]ionic forces[blank_end]. Binary compounds composed of two nonmetals or metalloids are generally molecular and are named using prefixes in the order designated by the formula.
The first element is named using the element’s name. The second element is written by using the stem name of the element with the suffix “ide” added.
[blank_start]2[blank_end] [blank_start]di[blank_end]
[blank_start]3[blank_end] [blank_start]tri[blank_end]
[blank_start]4[blank_end] [blank_start]tetra[blank_end]
[blank_start]5[blank_end] [blank_start]penta[blank_end]
[blank_start]6[blank_end] [blank_start]hexa[blank_end]
[blank_start]7[blank_end] [blank_start]hepta[blank_end]
[blank_start]8[blank_end] [blank_start]octa[blank_end]
[blank_start]9[blank_end] [blank_start]nona[blank_end]
[blank_start]10[blank_end] [blank_start]deca[blank_end]- ABinary compounds
- BIonic binary compounds
- Cionic forces
- D2
- Edi
- F3
- Gtri
- H4
- Itetra
- J5
- Kpenta
- L6
- Mhexa
- N7
- Ohepta
- P8
- Qocta
- R9
- Snona
- T10
- Udeca
17A [blank_start]chemical equation[blank_end] is a symbolic representation of a chemical reaction using chemical formulas. In a chemical reaction, the [blank_start]reactants[blank_end], written on the left, are substances that initiate the reaction. In a chemical reaction, the [blank_start]products[blank_end], written on the right, are substances that result from the reaction.
- Achemical equation
- Breactants
- Cproducts
18[blank_start]Synthesis or combination[blank_end] reactions involve the combining of two or more substances to form one product.
[blank_start]Decomposition[blank_end] reactions occur when a substance produces two or more other substances during a chemical reaction.
[blank_start]Single replacement[blank_end] reactions occur when an element replaces an ion in a compound.
[blank_start]Double replacement or metathesis[blank_end] reactions occur when two compounds interact in such a manner that the cation of one compound replaces the cation of the other compound and vice versa. This includes [blank_start]Acid-Base Reactions[blank_end], but these reactions form a salt and water.
Strong acids and Bases:
Perchloric Acid [blank_start]HClO4[blank_end]
Lithium Hydroxide [blank_start]LiOH[blank_end]
Sulfuric Acid [blank_start]H2SO4[blank_end]
Sodium Hydroxide [blank_start]NaOH[blank_end]
Hydroiodic Acid [blank_start]HI[blank_end]
Calcium Hydroxide [blank_start]Ca(OH)2[blank_end]
Hydrobromic Acid [blank_start]HBr[blank_end]
Strontium Hydroxide [blank_start]Sr(OH)2[blank_end]
Hydrochloric Acid [blank_start]HCl[blank_end]
Barium Hydroxide [blank_start]Ba(OH)2[blank_end]
Nitric Acid [blank_start]HNO3[blank_end]
Potassium Hydroxide [blank_start]KOH[blank_end]
[blank_start]REDOX reactions[blank_end] involve the transfer of electrons. The oxidation states should be determined in the reactants and the products.
[blank_start]Combustion[blank_end] reaction: Hydrocarbons react with oxygen to produce carbon dioxide and water.- ASynthesis or combination
- BREDOX reactions
- CCombustion
- DHClO4
- ELiOH
- FH2SO4
- GNaOH
- HHI
- ICa(OH)2
- JHBr
- KSr(OH)2
- LHCl
- MBa(OH)2
- NHNO3
- OKOH
- PDecomposition
- QSingle replacement
- RDouble replacement or metathesis
- SAcid-Base Reactions
19[blank_start]Molecular[blank_end] mass is the sum of the [blank_start]atomic[blank_end] masses of the atoms in a molecule of a substance.
- AMolecular
- Batomic
20The [blank_start]mole[blank_end] is a convenient way of dealing with a large number of molecules, atoms, ions, etc. The [blank_start]mole is[blank_end] abbreviated as “[blank_start]mol[blank_end].” This number is known as [blank_start]Avogadro’s[blank_end] number and is equal to [blank_start]6.0221367 x 10^23.[blank_end]
- Amole
- Bmole is
- Cmol
- DAvogadro’s
- EAvocado's
- F6.0221367 x 10^23.
- G6.023 x 10^24
21The [blank_start]percentage composition[blank_end] is the [blank_start]mass[blank_end] percentage of [blank_start]constituent elements[blank_end] that comprise the compound. Dividing the [blank_start]atomic mass[blank_end] of the [blank_start]compound[blank_end] into the [blank_start]atomic masses[blank_end] of [blank_start]the constituent elements[blank_end] and multiplying by 100 gives the percent composition of the compound. The percent composition totals 100%.
- Apercentage composition
- Bmass
- Cconstituent elements
- Datomic mass
- Ecompound
- Fatomic masses
- Gthe constituent elements
22The [blank_start]empirical[blank_end] formula shows the ratios of the number of [blank_start]atoms[blank_end] in the molecule; therefore, [blank_start]the empirical formula[blank_end] provides the relative number of each atom in a [blank_start]molecule[blank_end] of a substance.
The [blank_start]molecular[blank_end] formula is a whole number, n, multiple of the [blank_start]empirical formula[blank_end].- Aempirical
- Bmolecular
- Cempirical formula
- Datoms
- Ethe empirical formula
- Fmolecule
23When a chemical equation is balanced, the coefficients in front of the reactants and products are referred to as the [blank_start]stoichiometry[blank_end] of the chemical equation.
- Astoichiometry
- Breagents
24In a reaction vessel in which moles of quantity may be added without regard to the stoichiometry of the chemical process, the experimenter must be able to determine which quantity of materials will be in [blank_start]excess[blank_end] and which will be the [blank_start]right[blank_end] amount based on the balanced chemical equation.
- Aexcess
- Bdemand
- Cright
- Dwrong
25The [blank_start]theoretical[blank_end] yield is the maximum amount of product that can be obtained by a reaction from a given amount of reactants.
The [blank_start]percent[blank_end] yield is the amount of a substance obtained during an experimental process divided by the [blank_start]theoretical yield[blank_end] times 100.- Atheoretical
- Bpercent
- Ctheoretical yield
26[blank_start]Molarity[blank_end] is defined as the number of moles of a substance divided by the number of liters of solution.
[blank_start]Dilution[blank_end]:
M(before dilution) x V(before dilution) = M(after dilution) x V(after dilution)- AMolarity
- BDilution
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- Beschreibung
- N/A Old stuff Quiz am Quiz 2 study help, erstellt von Nathaniel Parkinson am 12/02/2021.
- Autor
- Nathaniel Parkinson
- Sprache
- English
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