2 1 units introduction
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This document discusses the importance of units in measurements and calculations. It introduces the seven standard base units used in science for measurements like length, mass, time, etc. Derived units are also explained as combinations of base units, like square meters for area or joules for energy. The document emphasizes that including units is crucial for chemistry calculations to catch mistakes, and advises writing out work on paper with units rather than solely using a calculator.
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This document provides guidance for students on scientific units, unit conversions, prefixes, and scientific notation. It begins with sample problems converting between time, mass, and length units. It then defines SI units and contrasts them with imperial units. Key points covered include the definitions of precision and accuracy, examples of unit prefixes like centi- and kilo-, and how to write numbers in scientific notation. Students are directed to complete practice problems and worksheets to reinforce these concepts.
Distance learning drilling_calculations_part_1 (1)
This document is an introduction to Part 1 of an IWCF UK Branch distance learning programme on drilling calculations. It provides an overview of the training objectives, which are to teach basic mathematical concepts and calculations required for working in the oil industry. It explains how to use the self-paced training programme, including how the material is organized into sections and laying out a sample study schedule. It also provides guidance on effective study habits.
Hc cs01 introduction_tochemistry
This document provides an overview of key chemistry concepts including the metric system, SI units, measurement and significant figures. It defines common metric prefixes and explains how to convert between metric units and base units. It also outlines best practices for taking measurements and recording results, including reading meniscus levels and recording uncertainty. Significant figure rules are summarized for determining the precision of data. Finally, tips are provided for effectively studying chemistry, such as memorizing terms and concepts, practicing algebra, and understanding patterns and connections between topics.
L2- AS-1 Physical quantities and units.pptx
1. A physical quantity is a quantity that can be measured and consists of a numerical magnitude and a unit. There are two types of physical quantities: base quantities and derived quantities.
2. The seven base quantities in the International System of Units (SI) are length, mass, time, current, temperature, amount of substance and luminous intensity. Common base units include the meter, kilogram and second.
3. Measurements have uncertainty due to random and systematic errors. Random errors cause unpredictable fluctuations while systematic errors arise from faulty instruments or flawed methods. Precision refers to the closeness of repeated measurements while accuracy refers to how close measurements are to the true value.
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More from jwallach
Algebra Review for General Chemistry Placement
This document provides an algebra review covering manipulating algebraic equations to solve for unknown variables. It discusses adding, subtracting, multiplying, and dividing terms on both sides of equations. It also covers solving equations with exponents and variables in denominators. Examples are provided for each concept and worked out step-by-step. Readers are encouraged to practice these skills on sample equations. Key points are to manipulate both sides of an equation equally and be careful not to incorrectly change a variable from the denominator to the numerator.
Unit 4 1 orbitals introduction
Electrons in atoms occupy specific energy states called orbitals. Orbitals represent the region where an electron is most likely to be found within its energy state. For example, the orbital occupied by the single electron in a hydrogen atom is shown as a cloud indicating a higher probability of finding the electron in the darker regions. While common diagrams depict electrons orbiting the nucleus like planets, this is not an accurate model - electrons occupy probabilistic regions described by orbitals rather than following precise orbits.
Unit 1 1 algebra review
The document provides an algebra review on manipulating algebraic equations to solve for an unknown variable x. It covers topics such as: adding/subtracting numbers, multiplying/dividing numbers, using a combination of operations, dealing with x in the denominator, misconceptions to avoid, exponents, and practice problems. The review explains that any manipulation done to one side of an equation must also be done to the other side to solve for x. It provides examples of isolating the term containing x and then solving.
Unit 7 4 stoichiometry – limiting reactants
This document discusses limiting reactants in chemical reactions. It explains that:
1) When reactants are combined in non-balanced ratios, one reactant will be consumed fully while excess of the other remains, with the fully-consumed reactant being the limiting reactant.
2) To determine the limiting reactant, the amounts of each reactant are converted to amounts of product, and the reactant that produces the lower amount of product is the limiting reactant.
3) Examples are provided to demonstrate this concept, including reactions involving hydrogen, oxygen, wheels, pedals and frames to make tricycles. The document cautions against common misconceptions in determining the limiting reactant.
Unit 7 3 stoichiometry - mass
This document discusses how to perform stoichiometric calculations using mass quantities instead of moles. It explains that the coefficients in a balanced chemical equation represent mole ratios that can be used to convert between reactants and products. An example calculation shows how to determine the mass of oxygen gas needed to react with a given mass of hydrogen gas using mole-mass conversions and the mole ratio from the balanced equation. The document emphasizes that coefficients should only be used when converting between moles, not masses. It also provides a practice problem and solution to reinforce the multi-step calculation process.
Unit 7 2 stoichiometry - mole
Stoichiometry is the process of using the coefficients in a balanced chemical equation to mathematically relate the quantities of substances involved in a chemical reaction. An example shows how to use the mole ratios from a balanced equation to calculate the moles of oxygen needed for a given number of moles of hydrogen, and the moles of water that would be produced. Key aspects are setting up conversion factors using the mole ratios and canceling out the given amount to solve for the desired quantity. Practice problems demonstrate calculating unknown reactants or products from amounts of other substances in the reaction.
Unit 7 1 balancing equations
This document discusses balancing chemical equations by adding coefficients to obey the law of conservation of mass. It explains that chemical equations must have the same number and type of atoms on both sides. To balance equations, coefficients are added in front of chemical substances without changing formulas. Examples show balancing equations by adding coefficients to match elements such as hydrogen, oxygen, and carbon on both sides. The document warns against changing formulas instead of using coefficients and provides hints for balancing equations.
Hybridization
This document discusses hybrid orbital bonding theory. It explains that atomic orbitals alone cannot describe bonding in molecules like methane, where carbon forms four equivalent bonds arranged tetrahedrally. Carbon's atomic orbitals cannot account for this. The solution is that carbon's 2s and 3p orbitals hybridize to form four new equivalent sp3 hybrid orbitals oriented at 109.5 degrees, allowing carbon to form four sigma bonds to hydrogen in methane. Hybridization is determined by counting electron domains, with sp, sp2, and sp3 hybridization occurring for 2, 3, and 4 domains respectively. This model explains methane's bonding and tetrahedral structure.
VSEPR models
This document introduces valence shell electron pair repulsion (VSEPR) theory, which is used to predict the molecular geometry of molecules based on the number of electron domains around the central atom. It explains that electron pairs repel each other and will spread out as far as possible in three dimensions. The number of electron domains determines the domain geometry, while the molecular geometry is based only on the arrangement of bonding domains. Examples are used to demonstrate how to draw dot diagrams and determine the domain and molecular geometries. Non-bonding pairs can cause a difference between domain and molecular geometry. Common molecular geometries that result from different numbers of bonding domains are also outlined.
Lewis dot diagrams
Lewis dot diagrams show the localization of valence electrons in atoms and molecules. They are drawn by placing the chemical symbol of each atom and then arranging electrons around the symbols to achieve full octets. For molecules, the least electronegative atom is placed in the center and single bonds are drawn between atoms before distributing remaining electrons. The octet rule is followed to maximize each atom's valence electrons to 8, with exceptions for hydrogen and some other elements. Practice examples are provided to demonstrate drawing Lewis dot diagrams for different atoms and molecules.
Unit 5 8 acid nomenclature
- Acids are covalent compounds that release hydrogen ions in water. Their names are determined by specific nomenclature rules.
- There are two categories of acids: binary acids containing hydrogen and one other atom type, and oxy-acids containing hydrogen and a polyatomic ion.
- Binary acids are named with the prefix "hydro-" followed by the other atom's name ending in "-ic". Oxy-acids do not use "hydro-" and change the polyatomic ion's name ending to "-ic".
Unit 5 7 covalent nomenclature
This document provides information on naming covalent compounds:
1) It outlines the process for naming covalent compounds, which involves stating the number of atoms using prefixes, then the element names with the second element ending in "-ide".
2) It lists the prefixes used to indicate the number of atoms in a compound from 1 to 10.
3) It notes an exception where the "mono-" prefix is omitted when there is only one of the first atom in the formula.
The document includes examples of naming and writing formulas for covalent compounds.
Unit 5 6 polyatomic ions
This document discusses polyatomic ions, which are ions composed of multiple atoms bonded together. It begins by explaining that polyatomic ions form when groups of atoms gain or lose electrons to become electrically charged. The document then lists and defines several common polyatomic ions, including ammonium, nitrate, carbonate, sulfate, and phosphate ions. It provides examples of how to write chemical formulas for compounds containing polyatomic ions by balancing the charges on the constituent ions. The document emphasizes correctly identifying polyatomic ions and distinguishing them from similar-sounding monatomic ions. It includes practice problems for writing formulas and names of ionic compounds involving common polyatomic ions.
Unit 5 5 basic ionic nomenclature
Ionic compounds are named by combining the name of the metal cation and non-metal anion. The non-metal name ends in "-ide". For example, sodium nitride is named Na3N, not trisodium nitride. To write formulas from names, determine the ion charges and balance them. Some students incorrectly add prefixes like "tri-" instead of just writing the compound name. Practice naming and writing formulas of common ionic compounds to build skills in basic ionic nomenclature.
Unit 5 4 basic ionic compounds
- Ionic compounds form when ions combine in simple whole number ratios to make neutral compounds. For example, sodium (Na+) and chloride (Cl-) ions combine in a 1:1 ratio to form NaCl.
- Calcium (Ca2+) and nitride (N3-) ions combine in a 3:2 ratio to form Ca3N2 in order to balance the charges.
- When writing ionic formulas, always use the simplest ratio of ions and do not write out ion charges, as the compound is neutral. For example, write PbS2, not Pb2+S2-.
Unit 5 3 molecular masses and conversions
This document discusses how to calculate molar masses of compounds by adding together the atomic masses of each element in the compound. It provides examples of calculating the molar mass of (NH4)2S, P4O10, SiCl4, and Cu3(PO4)2. The document also explains how to perform calculations involving moles, mass, and numbers of molecules or formula units of compounds using dimensional analysis and molar mass values. Practice problems are included for calculating moles or mass given the other value.
Unit 5 2 determining if a compound is ionic or covalent
This document discusses how to identify if a substance contains ionic or covalent bonds. It states that if a substance contains a metal and one or more non-metals, it likely contains ionic bonds. If a substance contains all non-metals, it likely contains covalent bonds, with the exception of ammonium compounds which contain ionic bonds despite having no metals. The document provides examples to illustrate these rules and includes a practice problem for the reader.
Unit 5 1 compounds
This document discusses chemical formulas and how to determine the number of each type of atom present in a compound from its formula. It explains that subscripts indicate how many of each atom are in the compound. For example, in H2O there are two hydrogen atoms and one oxygen atom. If a subscript is missing, it is understood to be one. Compounds are formed when atoms combine. Practice problems are provided to have the reader determine the number of each atom in sample formulas.
Unit 4 4 periodic properties
This document discusses periodic trends and how an element's position on the periodic table can be used to predict its atomic radius, first ionization energy, and electron affinity. It states that atomic radius generally increases moving left and down the table. First ionization energy and electron affinity increase moving up and right on the table. The document provides examples of these trends and practices applying them to choose the larger/higher value atom between pairs. It also notes that non-metals are above and right of the stair-step line on the periodic table, while metals are below and left of this line.
Unit 4 3 orbital filling diagrams
This document discusses orbital filling diagrams, which show how electrons are arranged in orbitals within an atom. It defines orbitals as regions of space where electrons are most likely to be found, and notes that each orbital can hold up to two electrons. It describes the shapes of s, p, d and f orbitals and explains that s orbitals are spherical while p orbitals are dumbbell shaped. The document demonstrates how to draw orbital filling diagrams that show the placement of electrons in orbitals according to rules of electron configuration.
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Unit 5 2 determining if a compound is ionic or covalent
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ESR spectroscopy in liquid food and beverages.pptx
With increasing population, people need to rely on packaged food stuffs. Packaging of food materials requires the preservation of food. There are various methods for the treatment of food to preserve them and irradiation treatment of food is one of them. It is the most common and the most harmless method for the food preservation as it does not alter the necessary micronutrients of food materials. Although irradiated food doesn’t cause any harm to the human health but still the quality assessment of food is required to provide consumers with necessary information about the food. ESR spectroscopy is the most sophisticated way to investigate the quality of the food and the free radicals induced during the processing of the food. ESR spin trapping technique is useful for the detection of highly unstable radicals in the food. The antioxidant capability of liquid food and beverages in mainly performed by spin trapping technique.
在线办理(salfor毕业证书)索尔福德大学毕业证毕业完成信一模一样
学校原件一模一样【微信：741003700 】《(salfor毕业证书)索尔福德大学毕业证》【微信：741003700 】学位证，留信认证（真实可查，永久存档）原件一模一样纸张工艺/offer、雅思、外壳等材料/诚信可靠,可直接看成品样本，帮您解决无法毕业带来的各种难题！外壳，原版制作，诚信可靠，可直接看成品样本。行业标杆！精益求精，诚心合作，真诚制作！多年品质 ,按需精细制作，24小时接单,全套进口原装设备。十五年致力于帮助留学生解决难题，包您满意。
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Sharlene Leurig - Enabling Onsite Water Use with Net Zero Water
Sharlene Leurig - Enabling Onsite Water Use with Net Zero WaterTexas Alliance of Groundwater Districts
Presented at June 6-7 Texas Alliance of Groundwater Districts Business MeetingThe use of Nauplii and metanauplii artemia in aquaculture (brine shrimp).pptx
Although Artemia has been known to man for centuries, its use as a food for the culture of larval organisms apparently began only in the 1930s, when several investigators found that it made an excellent food for newly hatched fish larvae (Litvinenko et al., 2023). As aquaculture developed in the 1960s and ‘70s, the use of Artemia also became more widespread, due both to its convenience and to its nutritional value for larval organisms (Arenas-Pardo et al., 2024). The fact that Artemia dormant cysts can be stored for long periods in cans, and then used as an off-the-shelf food requiring only 24 h of incubation makes them the most convenient, least labor-intensive, live food available for aquaculture (Sorgeloos & Roubach, 2021). The nutritional value of Artemia, especially for marine organisms, is not constant, but varies both geographically and temporally. During the last decade, however, both the causes of Artemia nutritional variability and methods to improve poorquality Artemia have been identified (Loufi et al., 2024).
Brine shrimp (Artemia spp.) are used in marine aquaculture worldwide. Annually, more than 2,000 metric tons of dry cysts are used for cultivation of fish, crustacean, and shellfish larva. Brine shrimp are important to aquaculture because newly hatched brine shrimp nauplii (larvae) provide a food source for many fish fry (Mozanzadeh et al., 2021). Culture and harvesting of brine shrimp eggs represents another aspect of the aquaculture industry. Nauplii and metanauplii of Artemia, commonly known as brine shrimp, play a crucial role in aquaculture due to their nutritional value and suitability as live feed for many aquatic species, particularly in larval stages (Sorgeloos & Roubach, 2021).
Unlocking the mysteries of reproduction: Exploring fecundity and gonadosomati...
The pygmy halfbeak Dermogenys colletei, is known for its viviparous nature, this presents an intriguing case of relatively low fecundity, raising questions about potential compensatory reproductive strategies employed by this species. Our study delves into the examination of fecundity and the Gonadosomatic Index (GSI) in the Pygmy Halfbeak, D. colletei (Meisner, 2001), an intriguing viviparous fish indigenous to Sarawak, Borneo. We hypothesize that the Pygmy halfbeak, D. colletei, may exhibit unique reproductive adaptations to offset its low fecundity, thus enhancing its survival and fitness. To address this, we conducted a comprehensive study utilizing 28 mature female specimens of D. colletei, carefully measuring fecundity and GSI to shed light on the reproductive adaptations of this species. Our findings reveal that D. colletei indeed exhibits low fecundity, with a mean of 16.76 ± 2.01, and a mean GSI of 12.83 ± 1.27, providing crucial insights into the reproductive mechanisms at play in this species. These results underscore the existence of unique reproductive strategies in D. colletei, enabling its adaptation and persistence in Borneo's diverse aquatic ecosystems, and call for further ecological research to elucidate these mechanisms. This study lends to a better understanding of viviparous fish in Borneo and contributes to the broader field of aquatic ecology, enhancing our knowledge of species adaptations to unique ecological challenges.
EWOCS-I: The catalog of X-ray sources in Westerlund 1 from the Extended Weste...
Context. With a mass exceeding several 104 M⊙ and a rich and dense population of massive stars, supermassive young star clusters
represent the most massive star-forming environment that is dominated by the feedback from massive stars and gravitational interactions
among stars.
Aims. In this paper we present the Extended Westerlund 1 and 2 Open Clusters Survey (EWOCS) project, which aims to investigate
the influence of the starburst environment on the formation of stars and planets, and on the evolution of both low and high mass stars.
The primary targets of this project are Westerlund 1 and 2, the closest supermassive star clusters to the Sun.
Methods. The project is based primarily on recent observations conducted with the Chandra and JWST observatories. Specifically,
the Chandra survey of Westerlund 1 consists of 36 new ACIS-I observations, nearly co-pointed, for a total exposure time of 1 Msec.
Additionally, we included 8 archival Chandra/ACIS-S observations. This paper presents the resulting catalog of X-ray sources within
and around Westerlund 1. Sources were detected by combining various existing methods, and photon extraction and source validation
were carried out using the ACIS-Extract software.
Results. The EWOCS X-ray catalog comprises 5963 validated sources out of the 9420 initially provided to ACIS-Extract, reaching a
photon flux threshold of approximately 2 × 10−8 photons cm−2
s
−1
. The X-ray sources exhibit a highly concentrated spatial distribution,
with 1075 sources located within the central 1 arcmin. We have successfully detected X-ray emissions from 126 out of the 166 known
massive stars of the cluster, and we have collected over 71 000 photons from the magnetar CXO J164710.20-455217.
8.Isolation of pure cultures and preservation of cultures.pdf
Isolation of pure culture, its various method.
Thornton ESPP slides UK WW Network 4_6_24.pdf
ESPP presentation to EU Waste Water Network, 4th June 2024 “EU policies driving nutrient removal and recycling
and the revised UWWTD (Urban Waste Water Treatment Directive)”
The binding of cosmological structures by massless topological defects
Assuming spherical symmetry and weak field, it is shown that if one solves the Poisson equation or the Einstein field
equations sourced by a topological defect, i.e. a singularity of a very specific form, the result is a localized gravitational
field capable of driving flat rotation (i.e. Keplerian circular orbits at a constant speed for all radii) of test masses on a thin
spherical shell without any underlying mass. Moreover, a large-scale structure which exploits this solution by assembling
concentrically a number of such topological defects can establish a flat stellar or galactic rotation curve, and can also deflect
light in the same manner as an equipotential (isothermal) sphere. Thus, the need for dark matter or modified gravity theory is
mitigated, at least in part.
The debris of the ‘last major merger’ is dynamically young
The Milky Way’s (MW) inner stellar halo contains an [Fe/H]-rich component with highly eccentric orbits, often referred to as the
‘last major merger.’ Hypotheses for the origin of this component include Gaia-Sausage/Enceladus (GSE), where the progenitor
collided with the MW proto-disc 8–11 Gyr ago, and the Virgo Radial Merger (VRM), where the progenitor collided with the
MW disc within the last 3 Gyr. These two scenarios make different predictions about observable structure in local phase space,
because the morphology of debris depends on how long it has had to phase mix. The recently identified phase-space folds in Gaia
DR3 have positive caustic velocities, making them fundamentally different than the phase-mixed chevrons found in simulations
at late times. Roughly 20 per cent of the stars in the prograde local stellar halo are associated with the observed caustics. Based
on a simple phase-mixing model, the observed number of caustics are consistent with a merger that occurred 1–2 Gyr ago.
We also compare the observed phase-space distribution to FIRE-2 Latte simulations of GSE-like mergers, using a quantitative
measurement of phase mixing (2D causticality). The observed local phase-space distribution best matches the simulated data
1–2 Gyr after collision, and certainly not later than 3 Gyr. This is further evidence that the progenitor of the ‘last major merger’
did not collide with the MW proto-disc at early times, as is thought for the GSE, but instead collided with the MW disc within
the last few Gyr, consistent with the body of work surrounding the VRM.
Travis Hills' Endeavors in Minnesota: Fostering Environmental and Economic Pr...
Travis Hills of Minnesota developed a method to convert waste into high-value dry fertilizer, significantly enriching soil quality. By providing farmers with a valuable resource derived from waste, Travis Hills helps enhance farm profitability while promoting environmental stewardship. Travis Hills' sustainable practices lead to cost savings and increased revenue for farmers by improving resource efficiency and reducing waste.
Remote Sensing and Computational, Evolutionary, Supercomputing, and Intellige...
Remote Sensing and Computational, Evolutionary, Supercomputing, and Intellige...University of Maribor
Slides from talk:
Aleš Zamuda: Remote Sensing and Computational, Evolutionary, Supercomputing, and Intelligent Systems.
11th International Conference on Electrical, Electronics and Computer Engineering (IcETRAN), Niš, 3-6 June 2024
Inter-Society Networking Panel GRSS/MTT-S/CIS Panel Session: Promoting Connection and Cooperation
https://www.etran.rs/2024/en/home-english/Shallowest Oil Discovery of Turkiye.pptx
The Petroleum System of the Çukurova Field - the Shallowest Oil Discovery of Türkiye, Adana
3D Hybrid PIC simulation of the plasma expansion (ISSS-14)
3D Particle-In-Cell (PIC) algorithm,
Plasma expansion in the dipole magnetic field.
Bob Reedy - Nitrate in Texas Groundwater.pdf
Presented at June 6-7 Texas Alliance of Groundwater Districts Business Meeting
Equivariant neural networks and representation theory
Or: Beyond linear.
Abstract: Equivariant neural networks are neural networks that incorporate symmetries. The nonlinear activation functions in these networks result in interesting nonlinear equivariant maps between simple representations, and motivate the key player of this talk: piecewise linear representation theory.
Disclaimer: No one is perfect, so please mind that there might be mistakes and typos.
dtubbenhauer@gmail.com
Corrected slides: dtubbenhauer.com/talks.html
Recently uploaded (20)
ESR spectroscopy in liquid food and beverages.pptx
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Sharlene Leurig - Enabling Onsite Water Use with Net Zero Water
Sharlene Leurig - Enabling Onsite Water Use with Net Zero Water
The use of Nauplii and metanauplii artemia in aquaculture (brine shrimp).pptx
The use of Nauplii and metanauplii artemia in aquaculture (brine shrimp).pptx
Unlocking the mysteries of reproduction: Exploring fecundity and gonadosomati...
Unlocking the mysteries of reproduction: Exploring fecundity and gonadosomati...
EWOCS-I: The catalog of X-ray sources in Westerlund 1 from the Extended Weste...
EWOCS-I: The catalog of X-ray sources in Westerlund 1 from the Extended Weste...
8.Isolation of pure cultures and preservation of cultures.pdf
8.Isolation of pure cultures and preservation of cultures.pdf
The binding of cosmological structures by massless topological defects
The binding of cosmological structures by massless topological defects
The debris of the ‘last major merger’ is dynamically young
The debris of the ‘last major merger’ is dynamically young
Travis Hills' Endeavors in Minnesota: Fostering Environmental and Economic Pr...
Travis Hills' Endeavors in Minnesota: Fostering Environmental and Economic Pr...
Remote Sensing and Computational, Evolutionary, Supercomputing, and Intellige...
Remote Sensing and Computational, Evolutionary, Supercomputing, and Intellige...
3D Hybrid PIC simulation of the plasma expansion (ISSS-14)
3D Hybrid PIC simulation of the plasma expansion (ISSS-14)
Equivariant neural networks and representation theory
Equivariant neural networks and representation theory
2 1 units introduction
- 2. All measurements need units • If I said an object has a length of 10, would this make any sense? • We need a unit with every number: – Length = 10 inches – Length = 10 feet – Length = 10 meters • Writing a number without a unit makes it meaningless
- 3. Standard Units • In science, we like to use standard units so that everyone around the world understands the measurements • The following are the seven standard base units: Measurement Unit Abbreviation Length Meter m Mass Kilogram kg Time Second s Amount of Substance Mole mol Electric Current Ampere A Luminous intensity Candela Cd Temperature Kelvin K
- 4. Derived Units • Notice how there are only 7 standard units. These are sufficient to cover many more than 7 measurements when you combine the base units. Below are a some examples of derived units – units that are combinations of base units. There are many more than shown in the table. Measurement Derived Unit Abbreviation In base units Area Square meters 𝑚2 𝑚2 Energy Joule J 𝑘𝑔 ∙ 𝑚2 𝑠2 Pressure Pascal Pa 𝑘𝑔 𝑠2 ∙ 𝑚 Force Newton N 𝑘𝑔 ∙ 𝑚 𝑠2
- 5. Using Units in Chemistry • While they are certainly required in chemistry, units can also be very helpful. In calculations, if you are careful with your units, then it becomes easy to spot mistakes in your calculations. • As you go through the exercises in this and later units, you will see units used quite a bit. Pay attention to them and ensure that when you are doing calculations on your own that you incorporate units. • For Blackboard, when entering numbers in as answers to problems, you should not include units. The reason for this is that Blackboard can easily misinterpret a unit. You should still have them on your own paper with your calculation, just do not try to enter units in with the answers to the problems.
- 6. Misconception Alert! • Students like to use calculators instead of paper. They try to solve questions on the calculator without taking the time to write the work out on paper and show their units. • Unless you are a student who is pretty certain you will get an A in the course and can lay everything out in your head, you should have good habits in solving problems. Get your problem set-up on paper before you plug numbers into a calculator and ensure that your units are correct all the way through the calculation.