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General Chemistry Part 1

Total questions: 108

Worksheet time: 1hrs 19mins

Name
Class
Date
1.

Anything that occupy space and has mass

(a)  

2.

2 or more substance in varying ratio

(a)  

3.

each substance that combined retain their distinct properties

(a)  

4.

It can be separated to its pure substances by physical means of separation.

(a)  

5.

uniform all throughout

(a)  

6.

only one phase/single phase

(a)  

7.

not uniform, two or more distinct phase

(a)  

8.

definite composition and distinct properties

(a)  

9.

two or more combination of elements in fixed proportion.

(a)  

10.

this can be separated but not with the use of physical means, but by the other means.

(a)  

11.

simplest form, can no longer subdivide.

(a)  

12.

independent on the amount of matter present

(a)  

13.

dependent on the amount of matter present.

mass dependent.

(a)  

14.

which of the following can be compressed in the states of matter

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

15.

Very Rigid

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

16.

which of the following that has no effect, and cannot be compresed.

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

17.

the following is indefite shape and definite volume.

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

18.

INDEFINITE that takes the shape of the container and fills the volume of the container.

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

19.

the intermolecular force of attraction is very strong

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

20.

the intermolecular force of attraction is intermediate

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

21.

the intermolecular force of attraction is essentially none

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

22.

the movement of this matter is vibration

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

23.

the movement of this matter is gliding

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

24.

the movement of this matter is random

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

25.

Solid to Gas

(a)  

26.

Gas to Solid

(a)  

27.

Solid to Liquid

(a)  

28.

Liquid to Solid

(a)  

29.

Liquid to Gas

(a)  

30.

Gas to Liquid

(a)  

31.

what is the greek word of atoms?

(a)  

32.

ATOMOS means

(a)  

33.

Who names the term "atomos"

(a)  

34.

proposed the modern atomic theory

(a)  

35.

Which of the following is not a part of Dalton atomic theory

a)

Elements are composed of tiny indestructible atoms

b)

Atoms are alike for a given elements. different element contains different atom different properties

c)

Compounds are formed with the combination of two atoms of different elements

d)

Compounds are formed with the atoms combined in single numberical ratio

e)

NONE

36.

Who propose the Law of Conservation of mass?

a)

Antioine Levoisier

b)

Robert Malikan

c)

JJ Thomson

d)

James Chadwick

37.

Mass before is equal to the mass after

(a)  

38.

mass cannot be created nor destroyed

(a)  

39.

Law of constant composition

(a)  

40.

a chemical compound regardless of its source if chemical preparation always contains the same composition.

(a)  

41.

Law of Definite Composition is also known as:

(a)  

42.

if two elements formed more than 1 compound.

(a)  

43.

what law combined in fix mass with the smallest whole number ratio.

(a)  

44.

consistent with the last postulate of atomic theory by john dalton.

(a)  

45.

Experiment with cathode ray tube

(a)  

46.

deflect aways from negative plate towards positive

(a)  

47.

Cathode rays are ______ charge that eventually called ______

(a)  

48.

atom is a sea of positively charges with imbedded negatively charge

(a)  

49.

Oil Drop Experiment

(a)  

50.

able to determine the charge/mass ratio of electron

(a)  

51.

observe penetrating ray from CRT which are not deflected by a magnet and he called it xray

(a)  

52.

spontaneous decomposition of chemicals emitting very penetrating rays.

(a)  

53.

coined radioactiviity

(a)  

54.

they discovered polonium and radium

(a)  

55.

alpha scattering experiment

(a)  

56.

Thin Gold Foil Experiment and Nuclear atomic model

a)

ERNEST RUTHERFORD

b)

JAMES CHADWICK

c)

JOHN NEWLANDS

d)

JOHN NEWLAND

57.

Planetary Model

a)

NIEL BOHR

b)

ANTOINE LAVOISIER

c)

ROBERT MILIKAN

d)

HENREY MOSELEY

58.

Quantum Mechanical Model

a)

ERWIN SCHRODINGER

b)

JOHN NEWLANDS

c)

GLENN SEABORG

d)

JJ THOMPSON

59.

Discovered neutron

a)

JAMES CHADWICK

b)

JJ THOMPSON

c)

ERNEST RUTHERFORD

d)

ANTOINE LAVOISIER

60.

discovered the nucleus of the atom

a)

ERNEST RUTHERFORD

b)

JAMES CHADWICK

c)

JJ THOMPSON

d)

ATOINE LAVOISIER

61.

mass of the whole atom

(a)  

62.

sum of protons and neutrons

(a)  

63.

atoms of the same element having different mass

a)

ISOTOPES

b)

ISOTONES

c)

ISOBAR

64.

atoms of the same # of neutrons

a)

ISOTOPES

b)

ISOTONES

c)

ISOBAR

65.

different elements having same mass

a)

ISOTOPES

b)

ISOTONES

c)

ISOBAR

66.

1 mole =

a)

AVOGADRO NUMBER 6.02 x 10 ^23

b)

AVOGADRO NUMBER 6.05 x 10 ^23

c)

AVOGADRO NUMBER 6.03 x 10 ^23

d)

AVOGADRO NUMBER 6.20 x 10 ^22

67.

Size of atom, location of electrons from nucleus. it main determinant of electrons energy.

a)

PRINCIPAL QUANTUM NUMBER

b)

ANGULAR MOMENTUM

c)

MAGNETIC QUANTUM NUMBER

d)

MAGNETIC SPIN

68.

Shape of orbitals

a)

ANGULAR MOMENTUM

b)

PRINCIPAL QUANTUM NUMBER

c)

MAGNETIC QUANTUM NUMBER

d)

MAGNETIC SPIN

69.

ORIENTATION IN SPACE

a)

MAGNETIC QUANTUM NUBER

b)

MAGNETIC SPIN

c)

ANGULAR MOMENTUM

d)

PRINCIPAL QUANTUM NUMBER

70.

+ 1/2 or -1/2

a)

MAGNETIC SPIN

b)

MAGNETIC QUANTUM NUMBER

c)

ANGULAR MOMENTUM

d)

PRINCIPAL QUANTUM NUMBER

71.

it is impossible to determine both the exact position and momentum of a particle

a)

HEISENBERG UNCERTAINTY PRINCIPLE

b)

PAULI EXCLUSION PRINCIPLE

c)

AUFBAU PRINCIPLE

d)

HUND'S RULE

72.

no two electrons in an atom can have the same set of 4 quantum numbers

a)

PAULI'S EXCLUSION PRINCIPLE

b)

HEISENBERGE UNCERTAINTY PRINCIPLE

c)

AUFBAU PRINCIPLE

d)

HUND'S RULE

73.

building up principle, fill up electons from the lowest energy orbital

a)

AUFBAU PRINCIPLE

b)

HUND'S RULE

c)

HEISENBERG UNCERTAINTY PRINCIPLE

d)

PAULI'S EXCLUSION PRINCIPLE

74.

the most stable arrangement of electron in subshells –up first of parallel spin

a)

HUND'S RULE

b)

AUFBAU PRINCIPLE

c)

PAULI'S EXCLUSION PRINCIPLE

d)

HEISENBERG UNCERTAINTY PRINCIPLE

75.

unpaired electron; can behave like a magnet

a)

PARAMAGNETIC

b)

DIAMAGNETIC

76.

paired electrons

a)

PARAMAGNETIC

b)

DIAMAGNETIC

77.

Father of Modern Chemistry

a)

ANTOINE LAVOISIER

b)

ERNEST RUTHERFORD

c)

JAMES CHADWICK

d)

JJ THOMPSON

78.

involves the formation of elements

a)

DIRECT UNION/COMBINATION REACTION

b)

DECOMPOSITION

c)

SINGLE REPLACEMENT

d)

DOUBLE REPLACEMENT

79.

breakdown of complex substances into simpler substance.

a)

DIRECT UNION/COMBINATION REACTION

b)

DECOMPOSITION

c)

SINGLE REPLACEMENT

d)

DOUBLE REPLACEMENT

e)

REDOX

80.

Na + HCl --> H2 + NaCl

a)

DIRECT UNION/COMBINATION REACTION

b)

DECOMPOSITION

c)

SINGLE REPLACEMENT

d)

DOUBLE REPLACEMENT

e)

REDOX

81.

causing chemical change by passing electricity through conducting solution

a)

ELECTROLYSIS

b)

HYDROLYSIS

c)

NEUTRALIZATION

d)

COMBUSTION

82.

NaCL + AgNO3 --> AgCl + NaNO3

a)

DIRECT UNION/COMBINATION REACTION

b)

DECOMPOSITION

c)

SINGLE REPLACEMENT

d)

DOUBLE REPLACEMENT

e)

REDOX

83.

the reaction between acid & a base to form salt & water

a)

ELECTROLYSIS

b)

HYDROLYSIS

c)

NEUTRALIZATION

d)

COMBUSTION

84.

Elements in free, uncombined state (diatomic found in nature) has zero net charge

a)

DIRECT UNION/COMBINATION REACTION

b)

DECOMPOSITION

c)

SINGLE REPLACEMENT

d)

DOUBLE REPLACEMENT

e)

REDOX

85.

Monoatomic ions have charges  Sum of all oxidation number is Zero if it is neutral and charge for those that are ions

a)

DIRECT UNION/COMBINATION REACTION

b)

DECOMPOSITION

c)

SINGLE REPLACEMENT

d)

DOUBLE REPLACEMENT

e)

REDOX

86.

Very Rigid

a)

SOLID

b)

LIQUID

c)

GAS

d)

PLASMA

87.

first extensive list of elementes

a)

Antoine Lavoisier

b)

Jons Jakob Berzelius

c)

Henry Moseley

d)

ERWIN SCHRODINGER

88.

table of atomic weight; letters as symbol

a)

Jons Jakob Berzelius

b)

Henry Moseley

c)

Glenn Seaborg

d)

Dmitri Mendeleev

89.

Law of Triads – average weight of ast and 3 rd element approximates that of the 2nd element and even their properties

a)

Johann Dobereiner

b)

Antoine Lavoisier

c)

Henry Moseley

d)

Glenn Seaborg

e)

JJ Thompson

90.

Law of octaves

a)

Johann Dobereiner

b)

Antoine Lavoisier

c)

Henry Moseley

d)

Glenn Seaborg

e)

John Newlands

91.

Father of periodic table

a)

Johann Dobereiner

b)

Dmitri Mendeleev

c)

Henry Moseley

d)

Glenn Seaborg

e)

John Newlands

92.

First periodic Law– according to increasing atomic weights

a)

Johann Dobereiner

b)

Dmitri Mendeleev

c)

Henry Moseley

d)

Glenn Seaborg

e)

John Newlands

93.

also work with First periodic law

a)

Johann Dobereiner

b)

Dmitri Mendeleev

c)

Lothar Meyer

d)

Glenn Seaborg

e)

John Newlands

94.

modify periodic law to increasing atomic number instead of weights

a)

Johann Dobereiner

b)

Dmitri Mendeleev

c)

Henry Moseley

d)

Glenn Seaborg

e)

John Newlands

95.

discovered transuramic elements and placed lanthanides above actinide; Seabrogium

a)

Johann Dobereiner

b)

Dmitri Mendeleev

c)

Henry Moseley

d)

Glenn Seaborg

e)

John Newlands

96.

The Periodical Table: Period

a)

HORIZONTAL

b)

VERTICAL

c)

Represent elements in s and p

d)

Represent d and f

97.

The Periodical Table: Group/Family

a)

HORIZONTAL

b)

VERTICAL

c)

Represent elements in s and p

d)

Represent d and f

98.

The Periodic table: A--->

a)

HORIZONTAL

b)

VERTICAL

c)

Represent elements in s and p

d)

Represent d and f

99.

The Periodic table: B--->

a)

HORIZONTAL

b)

VERTICAL

c)

Represent elements in s and p

d)

Represent d and f

100.

½ the distance between 2 nucleus in 2 adjacent atoms

a)

Atomic Radius

b)

Ionization Energy

c)

Electron Affinity

d)

Atomic Mass

101.

amount of energy required to remove an electron from neutral atom to form positive atom

a)

Atomic Radius

b)

Ionization Energy

c)

Electron Affinity

d)

Atomic Mass

102.

amount of energy release when a neutral atom accepts an electron to form a negative ion; can be measured

a)

Atomic Radius

b)

Ionization Energy

c)

Electron Affinity

d)

Atomic Mass

103.

this are smaller than their parent atomic radius

(a)  

104.

this are bigger than their parent atomic radius

(a)  

105.

reduction takes place

(a)  

106.

oxidation takes place

(a)  

107.

ability of an atom to attract electron to itself to form bond; can only be approximate; same trend as EA and IE

a)

Electronegativity

b)

Ionization energy

c)

Electron affinity

d)

Atomic radius

108.

is a space with certain area where mass is concentrated and that area is called nucleus

(a)  

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