what types of elements are ionic compounds made of
metal and nonmetal
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how do ionic compounds form
electrons are transferred from one atom to the other to form a cation and an anion that are attracted to each other with electrostatic attraction and form a giant crystal lattice of cations and anions with fixed electrons
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formula for lead nitrate
Pb(NO3)2
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formula for ammonium chloride
NH4Cl
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formula for potassium hydrocarbonate
KHCO3
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formula for copper (II) bromide
CuBr2
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formula for chromium (III) sulfate
Cr2(SO4)3
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Sn3(PO4)2
Tin phosphate
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Hg2S
Mercury sulfide
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what happens to the electron configurations of Mg and Br when they react to form the compound magnesium bromide
2 electrons transfer from magnesium to 2 bromide atoms to form a magnesium cation (Mg2+) and 2 bromide anions (2Br-) magnesium and bromide are attracted to each other through electrostatic attraction and form a giant crystal lattice Mg (1s22s22p63s2) Mg2+ (1s22s22p6) Br (1s22s22p63s23p64s23d104p5) Br- (1s22s22p63s23p64s23d104p6)
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what charge do cations have
positive charged ion remember ca+ion
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what charge does an anion have?
negatively charged ion
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why do some atoms have multiple charges?
fully filled, empty, and half-filled electron sublevels are more stable than partially filled levels
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what structure do ionic compounds form
a giant crystal lattice NO INDIVIDUAL MOLECULES
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what structures do covalent compounds form
individual discrete molecules
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how do covalent bonds form
electrons are shared between nonmetals - partially = polar - equally = non-polar
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what electronegativity difference is a nonpolar covalent
0.0-0.4 electronegativity difference
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what electronegativity difference is polar covalent
0.4-2.1 electronegativity difference
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what electronegativity difference is ionic
2.1-4.0 electronegativity
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what are the physical properties of metals
malleable, ductile, conductors of electricity and heat, lustrous, alloys
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why are metals malleable
electrons are free-moving in the crystal lattice of cations which means with enough force the cations can be forced to slide past each other
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what kinds of ions are metals
cations
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why are metals ductile
metals have free moving e- with fixed cations, which menas with enough force the crystal lattics of fixed cations can be forced to move past one another, stretching metal into wires
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why are metals lustrous
metals have fixed cations with free moving e- when photons are shined on metals they do not penetrate fully throughout the structure and instead are bounced off of the free/delocalized e-
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what is the movement of electrons in metals
electrons are delocalized, free moving
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why are metals good conductors of electricity
metals always have moving charges, from the delocalized e- therefore these moving charges can be induced into moving a specific direction with an applied charge, inducting electricity
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why are metals good conductors of heat
metals have delocalized e- that do not require large amounts of energy to move them more within the structure
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what is heat
total kinetic energy
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what is temperature
average kinetic energy
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are ionic compounds (s) good conductors of electricity
no. solid ionic compounds are fixed in a giant crystal lattice which means that the localized electrons are not abel to be induced into moving a specific way
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are covalent compounds good conductors of electricity
no. all phases of matter of covalent compounds cannot conduct electricity because they have no charges
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what is the electrical conductivity of (aq)/(l) ionic compounds
can conduct in aqueous or liquid state because the giant crystal lattice is broken and the e- are no longer localized
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can covalent compounds conduct heat
covalent compounds have weak intramolecular forces that cause the e- to be localized, covalent compounds do not require a lot of energy to break these intramolecular forces, which is why tehy have low melting and boiling points
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what types of compounds have high mp/bp
metalllic and ionic
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what types of compounds have low mp/bp
covalent compounds
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how do melting points of metals change going across a period
melting point of metals go up
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explain the trend in melting points going from Titanium to Cobalt
melting point increases - metallic bonding strength increases BECAUSE - #ve- and the charge of cations increases - radius decreases
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how does the melting point of metals change going down a group
melting point goes down
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explain the trend of melting points from Berylium to Barium
melting point decreases - metallic bonding strength decreases BECAUSE - cation radius increases down the table - increased shielding effect - greater distance between the ve- and cation -> weaker attraction to ve- -> weaker metallic bond
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which atoms are most likely to form covalent bonds
nonmetal atoms that share e-
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how does bond length change compared to bond strength
as number of bonds increases bond strength increases and length decreases BECAUSE the nuber of shared electron pairs increases
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what is the octet rule
an atom must have 8 ve- to satisfy its valence shell
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which flouride is the most ionic.Why? A. NaF B. CsF C. MgF2 D. BaF2
CsF, Cesium flouride because Cs and F have the highest electronegativity difference. Cs is the metal the lowest electronegativity and F with the highest electronegativity higher electronegativity difference means that it is more ionic
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which pair of elements reacts most readily A. Li + Br2 B. Li + Cl2 C. K + Br2 D. K + Cl2
D. K + Cl2 The electronegativity difference between potassium and chloride is the highest
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you are given two white solids and one is an ionic compound. describe 3 tests to perform to determine which is ionic. explain.
try conducting electricity (ionic compounds as solids are unable to conduct electricity, the one that acts as an insulator as a solid is the ionic compound) try heating and melting (ionic compounds have high mp/bp, so it would be more difficult ot melt/boil) test solubility in water (ionic compounds have ions that are attracted to each other with electrostatic attraction that are attracted to the partial charges of water H2O)
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Which of the following bonds contains the shortest bond between carbon and oxygen? A. CO2 B. H3COCH3 C. CO D. CH3COOH
carbon monoxide. carbon and oxygen has a triple bond between them
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predict the bonds of C - H C - Cl which is more polar? (Table 8 of data booklet)
electronegativity difference between C - H = 2.6-2.2 = 0.4 nonpolar/polar (in between) electronegativity difference between C - Cl = 3.2-2.6 = 0.6 polar C - Cl is more polar
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how do you determine the molecular geometry?
from molecular formulas
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VSEPR Theory
pairs of e- orient themselves as far apart as possible from each other
a molecule of hydrogen and carbon containing 2+ bonds
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alkene
hydrocarbons with double bonds C2H2n
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alkyne
hydrocarbons with triple bonds CnH2n-2
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naming alkenes and alkynes
identify the longest chain of consecutive carbons locate the double bond, and number chain so the double bond is the lowest numberlocate and number the substituents
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identify the construction of 2-methylhepta-1,5-diene
CH2CH(CH3)CH2CH2CHCHCH3 2-methylhepta-1,5-diene
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properties of hydrocarbons
non-polar - only betwen C & H London dispersion forces - forces stronger with greater mass - forces weather with more branching
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how do london dispersion forces change
becomes stronger with greater mass becomes weaker with branching
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how does boiling point of hydrocarbons change
decreases with increased branching becuase the london dispersion forces become weaker and it is easier for heat (energy) to break the london disperion forces between molecules
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homologous series
- differ by a CH2 - physical properties: MP/BP increases as the mass increases (mass increases as number of carbons increases) - chemical properties: homologous series will have similar chemical properties due to similar types of bonds (but depends on the types of bonds)
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complete combustion of hydrocarbons
CxHy +O2 (g) - > CO2(g) + H2O (g) + Energy
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type of reaction of combustion of hydrocarbons
exothermic, releases energy
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what state of matter when number of carbons 4
CxHy - gas
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what state of matter when number of carbons 5 >/=
CxHy - liquid
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CxHy - liquid
what state of matter when number of carbons 5 >/=
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how does incomplete combustion of hydrocarbons occur?
when there is insufficient oxygen O2
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products of incomplete combustion of hydrocarbons
soot, carbon monoxide
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what is the hazard of products of incomplete combustion of hydrocarbons
carbon monoxide - odorless, poisonous, results in carbon monoxide poisoning soot - can cause lung damage
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functional group
site of reactivity in a molecule - an atom or group of atoms
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class
= type or family of compounds containing a specific functional group
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alkanes, alkenes, alkynes, arene type of bonding (with only C and H)
non-polar covalent
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alkanes, alkenes, alkynes, arene type of IMF (with only C and H)
London Dispersion Forces ONLY
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alkanes, alkenes, alkynes, arene physical properties (with only C and H)
very volatile (can evaporate easily) high vapor pressure insoluable in water neutral
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