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Chemistry 103 > Quiz 1 > Flashcards

Quiz 1 Flashcards

1
Q

The atomic theory

A

1- Elements are composed of extremely small particles called atoms 

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2
Q

The atomic theory

A

All atoms of one element are identical, have the same size, mass and chemical properties 

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3
Q

The atomic theory

A

Compounds are composed of atoms of more than one element

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4
Q

The atomic theory

A

A chemical reaction involves only the separation combination or rearrangements of atoms. It does not result in their creation or destruction (law of conservation of mass)

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5
Q

Compounds

A

The same element can make different compounds differ in their number of atoms of each kind of that combine

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6
Q

The structure of the atom

A

Atoms are made of small particles called subatomic particles ; electrons, protons, and neutrons

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7
Q

Electron location

A

Outside the nucleus

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8
Q

Proton and neutron location

A

Inside the nucleus

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9
Q

The atomic number ( Z )

A

The number of protons in the nucleus of each atom of an element

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10
Q

The atomic number ( Z )

A

Atoms can be identified by the number of protons and neutrons, they contain

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11
Q

The atomic number ( Z )

A

The chemical identity of an atom can be determined from its atomic number 

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12
Q

The mass number ( A )

A

The total number of neutrons and protons present in the nucleus of an atom of an element 

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13
Q

The mass number ( A )

A

All atom nuclear contain both protons and neutrons. except for hydrogen, which has one proton and no neutrons 

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14
Q

Nucleons

A

Protons and neutrons are called nucleons

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15
Q

Neutron No.

A

The number of neutrons in an atom is equal to the difference between the mass number and the atomic number or ( A - Z )

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16
Q

Isotopes

A

Atoms that have the same atomic number, but different mass numbers due to the difference in neutron number 

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17
Q

Periodic table

A

A chart in which elements having similar chemical and physical properties are grouped together

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18
Q

Periodic table

A

Elements are arranged by atomic number in horizontal rows called periods and in vertical columns known as groups or families 

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19
Q

Periodic table

A

Elements are divided into three categories; metals, nonmetals and metalloids

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20
Q

Metal elements

A

A metal is a good conductor of heat and electricity 

21
Q

none metal elements

A

Nonmetal is a poor conductor of heat and electricity

22
Q

Metalloids

A

A metalloid has properties that are intermediate between those of metals and nonmetals

23
Q

Groups special names

A

Group 1A elements are called alkali metals
Group 2A elements are called alkaline earth metals
Group 7A elements are called halogens
Group 8A elements are called noble gases or rare gases

24
Q

Molecules

A

An aggregate of at least two atoms in a definite arrangement held together by chemical forces 

25
Q

Compounds

A

Is made up of two or more elements. Thus, all compounds are molecules, but not all molecules are compounds 

26
Q

Diatomic molecules

A

Molecules that contain only two atoms. it can be two atoms of the same element or two atoms of different elements 
H2 - HCl

27
Q

Polyatomic molecules

A

Molecules that contains more than two atoms, they can be atoms of the same element or a combination of two or more different elements 
O3 - NH3

28
Q

Homonuclear molecules

A

Molecule is composed of only one type of elements
O3 - H2

29
Q

Heteronuclear molecules

A

Molecules composed of more than one type of elements
HCl - CO2

30
Q

Ions

A

An atom or a group of atoms that has a net positive or negative charge

31
Q

Cation

A

The loss of one or more electrons from a neutral atom 

32
Q

Anion

A

The gain of one or more electrons from a neutral atom 

33
Q

Monatomic ions

A

Single atoms that gain or lose more than one electron

34
Q

Ions

A

Metals tend to form cations and nonmetals form anions

35
Q

Polyatomic ions 

A

Ammonium NH4+
Carbonate CO3 ^2 -
Cyanide CN-
Nitrate NO3-
Hydroxide OH-
Permanganate MnO4 -
Phosphate PO4 ^3-
Sulphate SO4 ^2-

36
Q

Molecular formula

A

A Formula which shows the exact number of atoms of each element in the smallest unit of a substance. It tells the actual number of atoms in a molecule 

37
Q

Structural formula

A

Shows how atoms are bonded to one another in a molecule
H — O — H

38
Q

Empirical formulas

A

The simplest chemical formulas they are written by reducing the subscript in the molecular formulas to the smallest possible number 
Molecular formula : H2O2
Empirical formula : HO

39
Q

ionic compounds

A

Chemical compounds composed of ions held together by electrostatic forces called ionic bonding. The compound overall is neutral, but consist of cations and anions. 

40
Q

Atomic mass

A

The mass of an atom depends on the number of electrons, protons and neutrons it contains

41
Q

Atomic mass

A

The mass of the atom in atomic mass units

42
Q

Mole

A

The amount of a substance that contains Avogadro’s number of entities

43
Q

Avogadro’s number

A

NA = 6.022*10^23

44
Q

Molar mass 

A

Molar mass = (atomic mass of atom X * number of atom X ) + ( atomic mass of atom Y * number of atom Y ) + … unit ( g/mol )

45
Q

Number of moles

A

Number of moles equals mass in grams divided by molar mass
n = m / M

46
Q

Number of particles

A

Number of particles equals Avogadro’s number times number of moles
N = NA * n

47
Q

The percent composition by mass

A

The percent by mass of each element in a compound

48
Q

Percent composition

A

Percent composition of an element equals number of Mars times molar mass of element divided by molar mass of compound times 100
Present composition = ( n * molar mass of element / molar mass of compound )* 100

Chemistry 103 (3 decks)

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