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CTLE Past Board Exam > General Chemistry > Flashcards

General Chemistry Flashcards

(64 cards)

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1
Q

He discovered the nucleus with his “Gold Foil” experiment.

A

Ernest Rutherford

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2
Q

He is credited with the discovery of electron in an atom.

A

J.J. Thomson

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3
Q

Which of the following is an intensive property?

A

Density

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4
Q

Which of the following is an extensive property?

A

Weight

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5
Q

Brass is an example of ___________.

A

Homogeneous mixture

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6
Q

Methane is an example of __________.

A

Compound

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7
Q

Which of the following is not an example of observable physical
property?

A

Mass

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8
Q

It is the number of proton in nucleus.

A

Atomic number

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9
Q

Atoms of the same element with varying number of neutrons

A

Isotopes

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9
Q

He formulated the Periodic Law.

A

Dmitri Mendeleev

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9
Q

He arranged the elements in the periodic table in groups of 8’s like
from lithium to sodium also known as “Law of Octaves”.

A

John Newlands

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9
Q

He arranged the elements in the periodic table in groups of 3’s or
triads also known as “Law of Triad”.

A

Johann Wolfgang Dobereiner

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10
Q

A substance that has the ability to dissolve or disperse one or more substances?

A

Solvent

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11
Q

A solution with solute that dissolves until it is unable to dissolve anymore, leaving the undissolved substances at the bottom.

A

Saturated solution

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12
Q

A solution that completely dissolves, leaving no remaining
substances.

A

Unsaturated solution

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13
Q

A solution that contains more undissolved solute than the saturated solution because of its tendency to crystallize and precipitate.

A

Supersaturated solution

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13
Q

Which of the following is arranged in increasing atomic size?

A

Mg > Ca > K > Fr

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14
Q

Which of the following elements is more electronegative: Cl, S, or
Mg?

A

Cl

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15
Q

Which of the following elements is more reactive: Li, Rb, or Fr?

A

Fr

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16
Q

The seven horizontal rows in the periodic table are called __________.

A

Periods

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17
Q

Group 7A is a family of _______

A

Halogens

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18
Q

It is the most ideal gas element.

A

Helium

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18
Q

These are properties that determine whether or not a substance will react chemically.

A

Chemical Properties (flammability, reactivity)

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18
Q

Which of the following elements (Br or Cu) has the higher ionization energy?

A

Br

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18
Which has a larger ionic size ( Na+ or Mg2+)
Na+
18
Sodium carbonate is also known as?
Soda ash
18
Agua regia is a/an ______.
solution
18
It does not depend on the size or amount of the sample.
Intensive Property (color, odor, boiling point)
19
These are properties that can be observed or measured.
Physical Properties (color, mass, length, volume, density, state, conductivity, temperature.)
19
Possible indication of chemical change:
1. Change in color 2. Change in temperature 3. Apperance or disappearance of precipitate 4. Evolution of gas
19
Each element is composed of extremely small particles called atoms.
Dalton’s Billiard Ball Model (1803)
19
The atom is made up of negative electrons that float in a sphere of positive charge like plums in a pudding. He discovered electron (cathode ray experiment).
Thomson’s Plum Pudding Model (1904)
19
Discovered the nucleus of a gold atom with his “gold foil” experiment.
Rutherford’s Nuclear Model (1911)
19
It depends on the size or amount of the sample.
Extensive Property (mass, volume)
20
Nucleus surrounded by orbiting electrons at different energy levels.
Bohr’s Planetary Model (1913)
20
He formulated the Periodic Law.
Dmitri Mendeleev
20
“Law of Octaves”
John Newlands
20
He recognized the repeating pattern or the periodic behavior among elements. He studied the relationship of the atomic volume and the relative atomic mass of 28 elements.
Julius Lothar Meyer
20
It is the average distance between nucleus and the valence electron.
Atomic Size (Atomic Radius)
20
“Law of Triad”
Johann Wolfgang Dobereiner
20
It is the ability of the atom to donate electrons.
Metallic Property
20
Cation Radius < Neutral Atomic Radius (Example: Al3+ < Al )
Anion Radius > Neutral Atomic Radius (Example: O2− > O )
20
It is the change in energy when an electron is accepted by a gaseous atom to form an anion.
Electron Affinity
20
It is tendency of an atom to react.
Reactivity
21
It is defined as the relative ability of an atom of an element to attract or gain electrons.
Electronegativity
21
Decreasing (top to bottom, right to left)
Ionization energy, electron affinity, electronegativity
21
It is the amount of energy required to remove an electron from an atom or ion.
Ionization Energy
21
Increasing (top to bottom, right to left)
Atomic size, metallic property, reactivity
22
It tells the shape of the orbital.
Azimuthal / Angular Momentum Quantum Number (l)
22
The average distance of the electron from the nucleus in a particular orbital.
Principal Quantum Number (n)
23
It describes the orientation of orbital.
Magnetic Quantum Number (ml)
23
It shows the spin of electrons.
Spin Quantum Number (ms)
23
Electron-transfer where one of the reacting atoms loses one or more electrons and the other atom gains on or more electrons. (metal to non-metal)
Ionic Bonding
23
It is formed by electron sharing, usually between atoms of non-metals. (non-metal to non-metal).
Covalent Bonding
24
The ratio of the total mass of each element to the total mass of one mole of the compound (MM) multiplied by 100%.
Percent Composition
24
Gives the actual ratio of the number of moles of atoms in a mole of the compound.
Molecular Formula
24
A mole is the amount of substance that contains Avogadro’s number of particles equal to 6.02x1023.
Avogadro's number
24
Ability of a solvent to dissolve a salt at a particular temperature.
Solubility
24
Solvent can still dissolve the solute.
Unsaturated Solution
24
Gives the simplest ratio of the number of moles of atoms.
Empirical Formula
25
If a solvent can’t no longer dissolve a given solute at a given temperature.
Saturated Solution
25
It is the sum of the atomic masses (in u) of all the atoms in a molecule.
Molecular Mass (amu)
25
It is the mass in grams of one mole of a substance.
Molar Mass (g/mol)
25
If the solvent can’t dissolve the solute and need to be heated for it to be dissolved.
Supersaturated Solution

CTLE Past Board Exam (9 decks)

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