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Section 1

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Charles' Law

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Chemistry Science

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Mar 1, 2020

Cards (46)

Section 1

(46 cards)

Charles' Law

Front

Volume and Temperature are directly proportional. V1/T1 = V2/T2

Back

Combined Gas Law

Front

Back

Mass Spectrometer

Front

1. Vaporization 2. Ionization 3. Acceleration 4. Deflection 5. Detection Mass/Charge Ratio, highest m/z deflects least, lowest m/z deflects most.

Back

What contains both ionic and covalent bonds?

Front

Any compound that contains a polyatomic ion! Example Sodium Hydroxide (NaOH)

Back

Properties of nonpolar substances

Front

Soluble in nonpolar solvent. Low M.P. b/c dispersion forces are weak. Does not conduct.

Back

Explain why S8 has a higher melting point than phosphorus P4.

Front

S8 is a larger macromolecular structure. Greater dispersion forces.

Back

Boyle's Law

Front

Pressure is inversely proportional to volume. P1V1 = P2V2

Back

Ionic Radius

Front

Cations are smaller than the atom from which it came. Anions are larger than the atom from which is came.

Back

Define Oxidation in terms or electron transfer

Front

Loses electrons

Back

Lewis definition of acid and base.

Front

Acid- electron pair acceptors. Base- electron pair donars.

Back

Properties of Metallic Solids

Front

Iron, Gold, Copper, Silver, etc. Not soluble High M.P. b/c metallic bonds are strong. Sea of electrons, can conduct as solid or molten.

Back

Explain why silicon has the highest melting point and argon has the lowest melting point?

Front

Silicon is a macromolecule with covalent bonds which require a lot of energy to break. Argon has lowest melting point because weakest dispersion forces.

Back

Arrhenius definition of acid and base.

Front

Acid- produces H+ (hydrogen ion or proton) in water Base- produces OH- (hydroxide) in water

Back

Acid-Base character of period 3 oxides

Front

Na, Mg: Basic Al: Amphoteric Si-Cl, Ar: Acidic Ar does not form an oxide.

Back

Emission of Hydrogen

Front

Emission: Energy levels 1 - 6 Lyman Series = UV Balmer Series = Visible Paschen = Infared

Back

Bronsred-Lowry definition of acid and base

Front

Acid- proton donar Base- proton acceptor

Back

Intermolecular Forces

Front

Hydrogen Bonding: H-O, H-F, H-N Dipole- Dipole Forces: Polar molecules Dispersion Forces: Weakest, nonpolar substances.

Back

What is meant be precision?

Front

Closeness of agreement of a set of measurements to each other. Consistency of measurement.

Back

Properties of ionic substnaces

Front

Soluble in polar solvent except things that form ppts. High M.P. b/c ionic bonds are strong. Conducts when molten or in aqueous solution. Do not conduct (not free moving).

Back

Melting points & reactivity for Halogens

Front

Down a group, m.p. increases. Reactivity increases going up, b/c electronegativity.

Back

Melting points & Reactivity for Alkali Metals

Front

Down group, m.p. decreases. Stronger metallic bonding. Reactivity increases down group.

Back

Strong acids (6)

Front

HCl H2SO4 HNO3 HClO4 HBr HI

Back

Properties of Network covalent solids

Front

Diamond (carbon) and Sand (SiO2) Not conductable.

Back

A X Z

Front

A= Mass number (# of protons and neutrons). Z= Atomic number (# of protons). X= Symbol of element.

Back

Define oxidation in terms of oxidation number.

Front

Oxidation number increases.

Back

Define average bond enthalpy

Front

Energy required to break 1 mole of a bond in a gaseous state. Average values obtained from a number of similar bonds.

Back

Properties of polar substances

Front

Soluble in polar solvent. Medium M.P. b/c Dipole-Dipole forces and hydrogen bonding. Usually nonconductor.

Back

Explain increase in melting point from Na to Al.

Front

Melting point increases because as cation becomes more positive since the radius decreases. More attraction for valence electrons.

Back

Covalent Bond

Front

Bonds formed as a result of shared electrons between 2 nonmetals. Nonpolar covalent- electrons are shared equally Polar covalent- electrons are not shared equally (more electronegative atom pulls on the e- more.) (Nonmetal w/ nonmetal: close --> nonpolar, far apart--> polar)

Back

Line Spectrum

Front

Discrete lines of electromagnetic radiation @ certain wavelength.

Back

Relationship between temperature and pressure

Front

Directly proportional.

Back

Define relative atomic mass.

Front

Average mass of isotopes of an element compared to average mass of an atom relative to C-12

Back

Electromagnetic Spectrum

Front

Wavelength and Frequency are indirectly proportional. Energy: E=hv

Back

Ionization Energy

Front

The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to produce 1 mole of gaseous ions with 1+ charge. X (g) --> X+ (g) + e- Decreases down a group - b/c atoms get larger, electrons move further from the nucleus so pull from nucleus is not as strong, it takes less energy to remove electron. Increases across period from left to right - atoms get smaller, nucleus has a strong hold on electrons, it takes more energy to remove it.

Back

Ionic Bond

Front

Electrostatic attraction between oppositely charged ions (metals with nonmetals).

Back

Properties of Group 8 solids

Front

Noble Gasses held together by dispersion forces. Not conductable.

Back

Define activation energy

Front

Minimum energy needed for a reaction to occur.

Back

Ideal Gas Law

Front

Back

Electronegativity

Front

Measure of the tendency of an atom to attract a bonding pair of electrons. Used to determine polarity of a bond.

Back

Continuous Spectrum

Front

Broad bands of electromagnetic radiation showing all colors over a wide range of wavelengths.

Back

Isotopes...

Front

Differ in mass, density, radioactivity, and stability. But they all have similar chemical properties, # of protons.

Back

Isotope

Front

An atom with the same number of protons but different mass number (number of neutrons).

Back

RAM

Front

Relative Atomic Mass % isotope1 (mass isotope1) + % isotope 2 (mass isotope 2)...

Back

Atomic Radius

Front

Increases down a group - size increases because electrons move further from nucleus since they are placed in higher energy levels. Decreases across a period from left to right - electrons are added to the same energy level, but there are more protons, so electrons get pulled closer to the nucleus making the atom smaller.

Back

Intramolecular Bonding

Front

Bonding within molecules. Covalent and ionic

Back

Avagadro's Principle

Front

Volume of gas is directly proportional to # of moles. V1/n = V2/n

Back