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Organic Chemistry > Matter and Atoms > Flashcards

Matter and Atoms Flashcards

Lesson 1 (42 cards)

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1
Q

study of carbon compounds with hydrogen, oxygen, nitrogen, etc.

A. Inorganic Chemistry
B. Chemistry
C. Organic Chemistry
D. Science

A

C. Organic Chemistry

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2
Q

simples form of matter made up of only 1 type of atom; examples: C, H, O, N, CI, Na, Ca, Fe, and Hg

A. Element
B. Matter
C. Compound
D. Molecule

A

A. Element

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3
Q

smallest particle of an element that retains the characteristics of the element

A. Metal
B. Molecule
C. Element
D. Atom

A

D. Atom

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4
Q

exhibits properties such as good conductivity of heat and electricity

A. metal
B. nonmetal
C. Atom
D. Acid

A

A. metal

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5
Q

poor conductors of heat and electricity, comprising of mostly organic chemistry

A. metal
B. nonmetal
C. Atom
D. Acid

A

B. nonmetal

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6
Q

composed of two or more elements in a specific ratio

A. mixture
B. compound
C. organic
D. molecule

A

B. compound

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7
Q

most likely to give electrons

A. metal
B. nonmetals
C. carbon
D. molecule

A

A. metal

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8
Q

any ___ containing compounds are organic

A. metal
B. nonmetals
C. carbon
D. molecule

A

C. carbon

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9
Q

a neutral group of atoms joined by covalent bond

A. metal
B. nonmetals
C. carbon
D. molecule

A

D. molecule

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10
Q

produces H+ in solution; examples – HCl, H2CO3, H3PO, and HC2H3O2

A. Salt
B. Acid
C. Base
D. Hydrogen

A

B. Acid

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11
Q

produces OHin solution; examples – NaOH, Ca(OH)2, and NH4OH

A. Salt
B. Acid
C. Base
D. Hydrogen

A

C. Base

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12
Q

neither acid nor base; produced by the reaction

A. Salt
B. Acid
C. Base
D. Hydrogen

A

A. Salt

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13
Q

Compounds can be classified as:

A. matter and element
B. metal and nonmetal
C. homogenous and heterogenous
D. inorganic and organic

A

D. inorganic and organic

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14
Q

consists of 2 or more substances physically combined in any portion by mass

A. Mixture
B. Inorganic
C. Compound
D. Organic

A

A. Mixture

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15
Q

mixture where components cannot be distinguised

A. homogenous mixture
B. heterogenous mixture
C. hemogenous mixture
D. heteragenous mixture

A

A. homogenous mixture

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16
Q

components can be distinguished after mixture

A. homogenous mixture
B. heterogenous mixture
C. hemogenous mixture
D. heteragenous mixture

A

B. heterogeneous mixture

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17
Q

atom is indivisible and indestructible

A. Bohr’s Atomic Model
B. Rutherford’s Nuclear Model of the Atom
C. Thomson’s Atomic Model
D. Dalton/s Atomic Theory

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A

D. Dalton’s Atomic Theory

18
Q

the atom is composed of a positively charged sphere embedded with electrons

A. Bohr’s Atomic Model
B. Rutherford’s Nuclear Model of the Atom
C. Thomson’s Atomic Model
D. Dalton/s Atomic Theory

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A

C. Thomson’s Atomic Theory

19
Q

the atom has a central dense part called the nucleus composed of protons and neutrons

A. Bohr’s Atomic Model
B. Rutherford’s Nuclear Model of the Atom
C. Thomson’s Atomic Model
D. Dalton/s Atomic Theory

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A

B. Rutherford’s Nuclear Model of the Atom

20
Q

the electrons in the atom surrounds the nucleus and are located in energy levels

A. Bohr’s Atomic Model
B. Rutherford’s Nuclear Model of the Atom
C. Thomson’s Atomic Model
D. Dalton/s Atomic Theory

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A

A. Bohr’s Atomic Model

21
Q

the electrons are specifically located in the orbitals of the sublevels, which make up the energy levels.

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A

Schrodinger’s Atomic Model

22
Q

refers to the distribution of electrons in the orbitals, sublevels, or subshells, and energy levels or shells of the atom.

A. Electron
B. Energy level
C. Electron Configuration
D. Sublevel

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A

C. Electron Configuration

23
Q

a space around the nucleus of an atom where an an electron is likely to be moving

A. Electron
B. Energy level
C. Electron Configuration
D. Sublevel

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A

B. Energy Level

24
Q

compose the energy level; designated as s, p, d, f, and so on

A. Orbitals
B. Energy level
C. Electron Configuration
D. Sublevel

25
the region in space where an electron stays most of the time A. Orbitals B. Energy level C. Electron Configuration D. Sublevel
A. Orbitals
26
spherical shape A. 3 p orbitals B. 1 s orbital C. 7 f orbitals D. 5 d orbitals
B. 1 s orbital
27
dumbell shape A. 3 p orbitals B. 1 s orbital C. 7 f orbitals D. 5 d orbitals
A. 3 p orbitals
28
clover leaf shape A. 3 p orbitals B. 1 s orbital C. 7 f orbitals D. 5 d orbitals
D. 5 d orbitals
29
complex shape A. 3 p orbitals B. 1 s orbital C. 7 f orbitals D. 5 d orbitals
C. 7 f orbitals
30
gives the numbers of electrons which is equal to the number of protons A. atomic number B. atomic mass C. atomic weight D. b or c
A. atomic number
31
gives the number of protons plus the number of electrons A. atomic number B. atomic mass C. atomic weight D. b or c
D. b or c
32
an arrangement of elements by increasing atomic number A. Group No. or Family No. B. Transition elements C. Period No. D. Periodic Table E. Representative Elements
D. Periodic Table
33
members of the 'A' families; have fixed oxidation states A. Group No. or Family No. B. Transition elements C. Period No. D. Periodic Table E. Representative Elements
E. Representative Elements
34
members of the 'B' families; have variable oxidation states A. Group No. or Family No. B. Transition elements C. Period No. D. Periodic Table E. Representative Elements
B. Transition Elements
35
elements belong to the same vertical arrangement; have the same number of valence electrons; have similar chemical properties A. Group No. or Family No. B. Transition elements C. Period No. D. Periodic Table E. Representative Elements
A. Group No. or Family No.
36
elements belong to the same horizontal arrangement; have the same number of energy levels A. Group No. or Family No. B. Transition elements C. Period No. D. Periodic Table E. Representative Elements
C. Period No.
37
the repetition of physical and chemical properties of the elements with increasing atomic number due to the reappearance of the same number of electrons in the outermost energy levels or shells of the atoms A. Electron Affinity B. Electronegativity C. Metallic Property D. Periodic Properties/Periodic Law E. Atomic Size/Radius
D. Periodic Properties / Periodic Law
38
metallic property decreases from left to right and increases from top to bottom A. Electron Affinity B. Electronegativity C. Metallic Property D. Periodic Properties/Periodic Law E. Atomic Size/Radius
C. Metallic Property
39
atomic size decreases from left to right and increases from top to bottom A. Electron Affinity B. Electronegativity C. Metallic Property D. Periodic Properties/Periodic Law E. Atomic Size/Radius
E. Atomic Size / Radius
40
amount of energy necessary to remove or dislodge an electron; ionization energy increases from left to right and decreases from top to bottom A. Electron Affinity B. Ionization Energy C. Metallic Property D. Periodic Properties/Periodic Law E. Atomic Size/Radius
B. Ionization Energy
41
energy released or absorbed when an atom gains an electron to form a negative ion; electron affinity increases from left to right and decreases from top to bottom A. Electron Affinity B. Ionization Energy C. Metallic Property D. Periodic Properties/Periodic Law E. Atomic Size/Radius
A. Electron Affinity
42
the tendency of an atom to attract electrons toward itself in a compound; electronegativity increases from left to right and decreases from top to bottom A. Electron Affinity B. Ionization Energy C. Electronegativity D. Periodic Properties/Periodic Law E. Atomic Size/Radius
C. Electronegativity

Organic Chemistry (2 decks)

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