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Chemistry > Chemistry Test 4 > Flashcards

Chemistry Test 4 Flashcards

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1
Q

Smallest particle of an element capable of chemical interactions

A

atom

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2
Q

Chemical compounds are composed of a fixed ratio of elements as determined by mass; there are always 2 hydrogens for 1 oxygen in a water molecule

A

law of definite proportions

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3
Q

streams of electrons that are produced when a high voltage is applied to electrodes in an evacuated tube; used by J.J. Thomson to find that every atom has small, negatively charged particles

A

cathode rays

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4
Q

A subatomic particle that has a negative charge; found outside the nucleus; has the least mass

A

electron

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5
Q

the center of an atom, which contains the protons and neutrons

A

nucleus

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6
Q

A subatomic particle that has a positive charge and that is found in the nucleus of an atom; aka atomic number; discovered by Ernest Rutherford

A

proton

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7
Q

the number of protons in the nucleus of an atom

A

atomic number (z)

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8
Q

A subatomic particle that has no charge and that is found in the nucleus of an atom; discovered by James Chadwick

A

neutron

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9
Q

the major energy levels of an atom (1-7); shells; first quantum number

A

principal energy level (n)

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10
Q

The lowest energy state of an atom

A

ground state

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11
Q

a packet of electromagnetic energy

A

photon

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12
Q

matter (including electrons) can be thought of as having properties of both a particle and a wave

A

Louis de Broglie

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13
Q

it is impossible to know exactly both the velocity and the position of a particle at the same time

A

Heisenberg uncertainty principle

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14
Q

a diagramic representation that uses dashes and arrows to show the principal energy levels and sublevels for all the electrons in an atom

A

orbital notation

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15
Q

Describes the subshell in which an electron is found; s, p, d, f

A

azimuthal quantum number (l)

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16
Q

the orientation of an orbital around the nucleus

A

magnetic quantum number (m)

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17
Q

The number that describes the two possible “spin” states of a pair of electrons in an orbital.

A

electron spin quantum number

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18
Q

two electrons in the same orbital must have opposite spins

A

Pauli exclusion principle

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19
Q

states that electrons must fill the lowest available energy sublevel before any can be placed in higher energy levels

A

Aufbau principle

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20
Q

the arrangement of electrons in an atom

A

electron configuration

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21
Q

electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible; describes how electrons fill orbitals

A

Hund’s rule

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22
Q

Atoms of the same element that have the same number of protons, but different numbers of neutrons

A

isotope

23
Q

the sum of the number of neutrons and protons in the nucleus

A

mass number (A)

24
Q

The representation of a specific isotope. The atomic number is listed below the symbol, the mass number above.

A

isotope notation

25
Q

alternative unit equivalent to the atomic mass unit

A

unified atomic mass unit (u)

26
Q

Electrons on the outermost energy level of an atom

A

valence electron

27
Q

an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol

A

electron dot notation

28
Q

A positively charged ion

A

cation

29
Q

A negatively charged ion

A

anion

30
Q

sublevel s can hold

A

2 electrons

31
Q

sublevel p can hold

A

6 electrons

32
Q

sublevel d can hold

A

10 electrons

33
Q

sublevel f can hold

A

14 electrons

34
Q

The modern periodic table is a model representing

A

principal energy levels and energy sublevels

35
Q

T/F The general region of space where an electron is most probably found is known as an orbital.

A

True

36
Q

T/F Neutrons contribute to an atom’s mass and its shape

A

False

37
Q

T/F An atom that gains three electrons will have a +3 charge

A

False

38
Q

T/F Electron dot notation is a shorthand way of showing valence electrons.

A

True

38
Q

T/F Each atom can be identified by the number of protons in its nucleus

A

True

39
Q

T/F No orbital can hold more than two electrons.

A

True

40
Q

T/F An electron can behave only as a wave.

A

False

41
Q

T/F The first quantum number identifies the principal energy level of an atom.

A

True

42
Q

T/F Scientific models are working representations of experimental facts that have been proven to be correct in all cases.

A

False

43
Q

determined by the weighted averages of isotopes of an element

A

Atomic mass

44
Q

Energy shells are also called

A

Energy levels

45
Q

The highest number of energy levels that atoms can have at ground state

A

7

46
Q

Philosophical atomism is a natural philosophy that proposes the universe is made up of indivisible particles called atoms. (Who discovered this?)

A

Democritus

47
Q

first experimental atomic model

A

John Dalton

48
Q

used the cathode ray tube to discover electrons; plum pudding model

A

J.J. Thomson

49
Q

discovered x-rays

A

Wilhelm Roentgen

50
Q

Discovered the neutron

A

James Chadwick

51
Q

conducted the gold foil experiment and discovered the alpha particle

A

Hans Geiger

52
Q

said that electrons are in energy levels; developed the planetary model

A

Niels Bohr

Chemistry (4 decks)

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