Regents Chemistry Megapack
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Regents Chemistry Megapack
Study 100 flashcards by ADMIN_. Use the interactive review above or scan this static preview for quick reference.
This flashcard set covers key concepts in chemistry, including definitions and applications of terminology such as STP, heat variables, and solubility tables. Learners will practice identifying various ion types, understanding chemical properties of elements, and calculating significant figures. Additional topics include atomic structure, bonding types, and periodic table trends, all aimed at enhancing foundational knowledge in chemistry.
Card 1
What does STP stand for in chemistry?
Standard Temperature and Pressure.
Card 2
What are heat variables for water used for?
Calculating needed energy for heat change.
Card 3
What are measurement prefixes used for?
For very small or large numbers.
Card 4
What do polyatomic ions act like?
They act like singular ions.
Card 5
How is solubility determined for a compound?
By checking if it contains listed ions with exceptions.
Card 6
What does a solubility table show?
Compounds' solubility based on temperature and water quantity.
Card 7
What determines if a liquid becomes a gas?
If pressure and temperature are above the liquid's line, it becomes a gas.
Card 8
What distinguishes endothermic and exothermic reactions?
Negative numbers are exothermic; positive numbers are endothermic.
Card 9
How is hydrogen unique among elements?
Hydrogen is not a metal but behaves like one.
Card 10
What ion is common in acids?
Acids have a hydrogen ion.
Card 11
What ion is common in bases?
Bases have a hydroxide (OH) ion.
Card 12
What do acid-base indicators do?
They change color based on pH range.
Card 13
What does a radioactive isotope table list?
Half-life, decay mode, isotopes.
Card 14
How are organic molecules named?
By prefixes based on carbon atom number.
Card 15
What do suffixes indicate in organic chemistry?
Type of bond: single, double, triple, and group affects properties.
Card 16
What are significant figures?
Defined as digits in a number contributing to its precision.
Card 17
How do you determine significant figures in a decimal?
Start left, count from first non-zero digit to end.
Card 18
How do you handle significant figures in addition?
Round result to the number with the fewest decimal places.
Card 19
How do significant figures affect rounding after addition?
The result is rounded to match the limiting term's decimal places.
Card 20
What happens if a number ends in zeroes without a decimal point?
Zeroes are not significant if there's no decimal point.
Card 21
What is the rule for significant figures when multiplying 30.0700 by 7.082?
Use the number with the fewest significant figures, which is 4.
Card 22
How many significant figures does the number 7.082 have?
4 significant figures.
Card 23
What is the process to round 212.95574 to the correct significant figures?
Round to 213.0 to have 4 significant figures.
Card 24
How many significant figures are in the number 200?
1 significant figure.
Card 25
What is the number of significant figures in 0304.80?
5 significant figures.
Card 26
How many significant figures does 0.00203980000 have?
9 significant figures.
Card 27
What is the correct number of significant figures for 8000.00003?
9 significant figures.
Card 28
What is the significance of trailing zeros without a decimal point?
They don't count if there's no decimal point.
Card 29
How is energy defined in chemistry?
It is the study of composition, structure, properties, and reactions of matter.
Card 30
What is considered 'not matter' in chemistry?
Energy, as it does not have mass and volume.
Card 31
What happens during an exothermic process?
Heat leaves an object.
Card 32
What occurs in an endothermic process?
Heat enters an object.
Card 33
What phase changes occur with increased heat?
Solids become liquids, then gases.
Card 34
How is pressure defined in the context of chemistry?
Pressure is the measure of force in an area.
Card 35
What is the formula for converting Celsius to Kelvin?
Add 273 to the Celsius temperature.
Card 36
What is the coldest possible temperature in Celsius?
-273C is the coldest temperature.
Card 37
What happens to kinetic and potential energy as ice melts to a liquid?
Kinetic energy doesn't increase; potential energy does.
Card 38
In an endothermic heat curve, how does energy change as a gas forms?
Energy absorbed by a gas increases in kinetic energy.
Card 39
What formula calculates the energy required to melt a block of ice?
Q = mHf is used to calculate the energy.
Card 40
What do the symbols in the formula Q = mHf represent?
Q is energy in joules, m is mass, Hf is Heat of Fusion.
Card 41
What amount of energy is required to melt 10g of ice?
3340 J
Card 42
What does q = mHv calculate?
The energy from liquid to gas or gas to liquid.
Card 43
What is the Heat of Vaporization of water?
2260 J/g
Card 44
How much energy is needed to evaporate 10g of water?
22600 J
Card 45
What does Q = mCT calculate?
The energy change with temperature change.
Card 46
What is the Specific Heat Capacity of water?
4.18 J/g*K
Card 47
How do you find the change in temperature in Q = mCT?
Subtract Temperature 1 from Temperature 2.
Card 48
What are the values for Standard Temperature and Pressure (STP)?
101.3 kPa or 1 atm for pressure, 273 K or 0C for temperature.
Card 49
What is the Celsius equivalent of 200 K?
-73C
Card 50
How many joules to turn 15g of water into a gas?
33900 J
Card 51
If 5678 J are used, how many grams of water are melted?
17g
Card 52
What is the formula for the Combined Gas Law?
(P1V1)/T1 = (P2V2)/T2
Card 53
How must temperatures be expressed in gas law calculations?
In Kelvin
Card 54
In the Combined Gas Law, what happens to volume if pressure and temperature increase?
Volume decreases.
Card 55
What conditions make a gas behave most like an ideal gas?
High temperatures and low pressures.
Card 56
What motion do ideal gas particles exhibit?
Random, rapid, constant straight-line motion.
Card 57
What are subatomic particles in an atom?
Protons, electrons, and neutrons.
Card 58
What defines the element of an atom?
Protons determine the element.
Card 59
What impact do electrons have on an atom or ion?
Determine how the atom or ion acts.
Card 60
What is the role of neutrons in an atom?
Neutrons have little impact, just present.
Card 61
What is an ion?
An ion is formed when there is a different number of electrons compared to protons.
Card 62
What are isotopes?
Isotopes are atoms with different numbers of neutrons compared to each other.
Card 63
Who proposed the 'Hard Sphere' model of the atom?
John Dalton proposed the 'Hard Sphere' model.
Card 64
What did Thomson's 'Plum Pudding' model declare?
Thomson's model declared that negatively charged particles are embedded in a larger positive charge.
Card 65
What was the conclusion of Rutherford's Gold Foil Experiment?
It concluded that atoms are mostly empty space with a small, dense, positive nucleus.
Card 66
What is the 'Planetary' model associated with?
The 'Planetary' model is associated with Bohr.
Card 67
What does the 'Wave Mechanical' model depict?
It depicts the most probable location for an electron as an orbital.
Card 68
Where are metals and nonmetals located on the periodic table?
Metals are on the left, and nonmetals are on the far right of the periodic table.
Card 69
What are periods and groups on the periodic table?
Periods are rows across; groups are columns down.
Card 70
What are alkali metals and alkali earth metals?
Alkali metals are in group 1; alkali earth metals are in group 2.
Card 71
What are noble gases and halogens?
Noble gases are in group 18; halogens in group 17.
Card 72
What properties do elements in the same group share?
Elements in the same group have similar chemical properties.
Card 73
What is an atomic number?
The atomic number is the number of protons in an element.
Card 74
What is atomic mass?
Atomic mass is the average mass number of all natural isotopes of an element.
Card 75
What is the significance of valence electrons?
Valence electrons determine reactivity and stability of an atom.
Card 76
How does oxygen form a water molecule with hydrogen?
Oxygen shares electrons with two hydrogens to form H2O.
Card 77
What is a double bond?
A double bond forms when two atoms share two electrons each.
Card 78
What are Lewis dot structures used for?
They are used to represent valence electrons in bonding.
Card 79
What do ionic dot structures represent?
They represent electron transfer in ionic bonds.
Card 80
What is the purpose of calculating the relative abundance of isotopes?
It helps determine the average atomic mass of an element.
Card 81
What is an isotope in terms of atomic structure?
An isotope is an atom of the same element with different numbers of neutrons.
Card 82
How do you calculate the relative atomic mass of a sample with isotopes?
Convert percentages to decimals, multiply by mass numbers, and add results.
Card 83
What happens to atomic radius as you go down a group on the periodic table?
The atomic radius increases as you go down a group.
Card 84
How does atomic radius change as you go across a period?
The atomic radius decreases as you go across a period.
Card 85
What is ionization energy and how does it change across the periodic table?
Ionization energy is the energy required to remove an electron; it decreases down a group and increases across a period.
Card 86
What is electronegativity and its trend on the periodic table?
Electronegativity is an atom's ability to attract electrons; it decreases down a group and increases across a period.
Card 87
What is metallic character and how does it change across the periodic table?
Metallic character indicates how much an element behaves like a metal; it increases down a group and decreases across a period.
Card 88
How does an atom become a cation or an anion?
An atom becomes a cation when it loses an electron and an anion when it gains one.
Card 89
What are the typical properties of metals?
Metals are shiny, conductive, malleable, ductile, solid at STP, and lose electrons.
Card 90
What properties do nonmetals typically have?
Nonmetals are dull, nonconductive, brittle, can be any phase at STP, and tend to gain or share electrons.
Card 91
What are metalloids and their properties?
Metalloids have properties of both metals and nonmetals.
Card 92
What is an electron configuration and give an example for silicon?
Electron configurations show the number of electrons in each shell; silicon is 2-8-4.
Card 93
What happens when electrons absorb energy in an atom?
Electrons absorb energy, move to higher levels, and release light when returning to ground state.
Card 94
What is the difference between covalent and ionic bonds?
Covalent bonds share electrons; ionic bonds transfer electrons.
Card 95
How are all compounds related to molecules?
All compounds are molecules, but not all molecules are compounds.
Card 96
How do sodium and chlorine form table salt?
Sodium donates an electron to chlorine, forming NaCl (table salt).
Card 97
What is a characteristic of compounds like magnesium bromide?
Magnesium bromide does not form a 1:1 ratio; it forms MgBr2.
Card 98
How do you determine the ratio of atoms in compounds like CaO?
The ratio is determined by matching the number of electrons each atom wants to transfer.
Card 99
What do oxidation states on the periodic table indicate?
Oxidation states indicate the electrons an atom will transfer.
Card 100
How is an element's name modified to indicate different oxidation states?
An element's name includes a Roman numeral to indicate different oxidation states.