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Honors Chemistry > Finals > Flashcards

Finals Flashcards

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1
Q

Electro negativity

A

The ability to attract electrons

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2
Q

Covalent bond in which the shared electron pair comes from only 1 of the atoms

A

Coordinate covalent bond

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3
Q

Covalent bond between two atoms of significantly different electronegativities

A

Polar bond

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4
Q

Type of bond that is very important in determining the properties of water and of important biological molecules (proteins and DNA)

A

Hydrogen bond

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5
Q

The number of grams of an element that is numerically equal to the atomic mass of the element in amu

A

Atomic mass

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6
Q

The volume occupied by a mole of any gas at STP

A

Molar volume

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7
Q

The number of representative particles of a substance present in 1 mile of that substance

A

Avogadro’s number (6.022*10^23)

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8
Q

An atom ion or molecule

A

Representative particle

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9
Q

0• C and 1 atm

A

STP

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10
Q

Percent by mass of each element in a compound

A

Percent composition

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11
Q

Smallest whole number ratio of atoms in a compound

A

Empirical formula

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12
Q

Combustion reaction

A

Reactant: oxygen gas

Product: carbon dioxide and water

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13
Q

Actual yield/theoretical yield*100

A

Percent yield

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14
Q

Characteristic of ionic compound

A

High melting point

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15
Q

How do atoms achieve noble gas configurations in single covalent bonds?

A

Two atoms share two electrons

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16
Q

According to the VESPAR theory, molecules adjust their shapes to keep which of the following as far apart as possible?

A

Pairs of valence electrons

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17
Q

What causes water molecules to have a bent shape?

A

Repulsive forces between unshared pairs of electrons

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18
Q

Weakest molecular attraction

Strongest

A

Dispersion

Hydrogen

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19
Q

How many liters are in a mole?

A

22.41 L

20
Q

How to find the density at STP of a gas?

A

Molecular weight/22.41 liters per mole

G/mole

21
Q

To find empirical formula…

A

Divide percent by molecular weight

Divided all by smallest number

22
Q

Double replacement reaction

A

Two ionic compounds

23
Q

How to figure out if single replacement reactions can take place

A

Activity series of metals (has to be higher above to replace it)

24
Q

Example of a driving force of a reaction

A

Precipitate is formed

25
Q

Basic solution contains a lot of____ions and is located where on the PH scale?

A

OH

8-14

26
Q

Acids contain a lot of____ions and is located where on the PH scale?

A

Hydrogen

Lower than 7

27
Q

S orbital

A

Spherical

28
Q

P orbital

A

Dumbbell

29
Q

4s2….

A

3d#

30
Q

Exceptions in the d block

A

d9 and d4 become d10 and d5

31
Q

Periodic trends

A

The atomic radius decreases from left to right and bottom to top while the electronegativity and ionization energy increase

32
Q

If a reaction is endothermic it has a____enthalpy

A

Positive

33
Q

Enthalpy of exothermic reaction

A

Negative

34
Q

Bronsted Lowry acid

A

A molecule or ion that is a donor

35
Q

Bronsted Lowry base

A

A molecule or ion that is a proton acceptor

36
Q

Conjugate base

A

Species that remains after a Bronsted Lowry acid has given up a proton

37
Q

Conjugate acid

A

Species that is formed when Bronsted Lowry base gains a proton

38
Q

When making a titration, the equivalence point represents when____

A

The moles of acid equal the moles of base

39
Q

Molality

A

Mole solute/kg solvent

40
Q

Ionization energy

A

Energy required to remove an electron

41
Q

99.7 MHz equals how many hertz

A

99.7*10^6 Hz

42
Q

Planks constant

A

3.00*10^8 m/s

43
Q

Unit for frequency

A

Hertz

44
Q

Unit for wavelength

A

Meters

1 meter=10^-9 nanometers

45
Q

In the equation for boiling point you can find the i value (ionic) by determining

A

How many things it breaks up into

NaCl=2

46
Q

Freezing point is always

A

Negative

Honors Chemistry (8 decks)

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